Chemistry11 Final Exam Review 2019 (2)
docx
keyboard_arrow_up
School
Western University *
*We aren’t endorsed by this school
Course
11
Subject
Chemistry
Date
Feb 20, 2024
Type
docx
Pages
15
Uploaded by UltraEchidnaPerson795
Chemistry 11
Course Review
Chemistry 11 – June Exam Review
Unit 1—
The Mole Concept
1. Make the following conversions, clearly showing your steps. Include proper units in all of your work and in your answer. a)
133.44 grams of PCl
5
= ? moles Answer ___________________________
b)
0.00256 moles of Li
2
Cr
2
O
7
= ? grams Answer ___________________________
c)
170.24 L of NO
2
at STP = ? moles Answer ___________________________
d)
570.625 g of PCl
3
gas = ? L (STP) Answer ___________________________
e)
1030.4 mL of C
2
H
6
gas at STP = ? g Answer ___________________________
f)
5.00 kg of nitrogen gas, N
2
= ? L (STP) Answer ___________________________
g)
0.5696 kg of CH
4(g)
= ? mL Answer ___________________________
Chemistry 11—Course Review
Page 1
Chemistry 11
Course Review
2.
The density of liquid ethanol (C
2
H
5
OH) is 0.790 g/mL. Calculate the number of molecules in a 35.0 mL sample of liquid ethanol. (NOTE: You CAN’T use 22.4 L/mol since this is NOT a gas at STP!)
Answer __________________________
3.
A 100.0 mL sample of liquid mercury contains 6.78 moles. Calculate the density of liquid mercury from this data.
Answer __________________________
4.
Calculate the density of PCl
3(g)
at STP.
Answer __________________________
5.
The density of a gas at STP is 4.955 g/L. Calculate the molar mass of this gas.
6.
123.11 g of zinc nitrate, Zn(NO
3
)
2
are dissolved in enough water to form 650.0 mL of solution. Calculate the [Zn(NO
3
)
2
]. Include proper units in your work and in your answers. Answer _______________________________
Chemistry 11—Course Review
Page 2
Chemistry 11
Course Review
7.
Calculate the mass of potassium sulphite (K
2
SO
3
) needed to make 800.0 mL of a 0.200 M solution of K
2
SO
3
. Include proper units in your work and in your answers.
Answer ______________________
8.
What volume of 2.50 M Li
2
CO
3
would need to be evaporated in order to obtain 47.232 g of solid Li
2
CO
3
? Include proper units in your work and in your answers. Answer ______________________
9.
150.0 mL of water are added to 400.0 mL of 0.45 M HNO
3
. Calculate the final [HNO
3
]. Include proper units in your work and in your answers. Answer ______________________
10.
What volume of water needs to be added to 150.0 mL of 4.00 M H
2
SO
4
in order to bring the concentration
down to 2.50 M? Include proper units in your work and in your answers. Answer ______________________
11.
Give directions on how to make 5.00 L of 0.020 M Ca(ClO)
2
using solid Ca(ClO)
2
and water. Include proper units in your work and in your answers. Directions:
Unit 2—
Chemical Reactions
1.
Balance the following equations NH
3
+ O
2
NO + H
2
O
(NH
4
)
2
C
2
O
4
+ AlCl
3
Al
2
(C
2
O
4
)
3
+ NH
4
Cl
C
14
H
30
+ O
2
CO
2
+ H
2
O
Chemistry 11—Course Review
Page 3
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Chemistry 11
Course Review
Fe + HNO
3
Fe(NO
3
)
3
+ H
2
P
4
+ Cl
2
PCl
3
H
3
PO
4
+ Ca(OH)
2
Ca
3
(PO
4
)
2
+ H
2
O
Ba(ClO
4
)
2
Ba + Cl
2
+ O
2
MgSO
4
.
5H
2
O
MgSO
4
+ H
2
O
2.
Write a balanced chemical equation for each of the following, and classify each as synthesis, decomposition, single replacement, double replacement, neutralization or combustion.
a)
potassium sulphate is mixed with cobalt (III) nitrate
b)
liquid propanol (C
3
H
7
OH) is burned in air
c)
ammonium nitrate is decomposed into it’s elements
d)
a piece of zinc is placed in a test-tube containing a solution of silver nitrate
e)
bromine reacts with sodium iodide
3.
State whether each of the following are exothermic
or endothermic
. HCl + 432 kJ
H + Cl
Answer ___________________________
C
12
H
22
O
11
+ 12 O
2
12CO
2
+ 11H
2
O
H = -5638 kJ Answer ___________________
H
2
O
(s)
H
2
O
(l)
Answer ___________________________
Answer ___________________________
CD
C + D
H= 65.7 kJ
Answer ___________________________
E + F + 437 kJ
G + H
Answer ___________________________
Chemistry 11—Course Review
Page 4
A + B
Energy (kJ)
Reaction Proceeding
AB
Chemistry 11
Course Review
4.
Given the equation: C
12
H
22
O
11
+ 12O
2
12CO
2
+ 11H
2
O + 5638 kJ
a.
How much heat is released during the formation of 880.0 g of CO
2
? Answer _____________________________
b.
How much heat is released during the formation of 5.6 moles of H
2
O? Answer _____________________________
c.
If 179.2 L of O
2
(STP) are consumed, how much heat is released? Answer _____________________________
5.
Calculate the amount of heat (in Joules) required to warm 200.0 g of water from 8.0
o
C to 45.0
o
C. (Heat Capacity (C) for H
2
O is 4180 J/kg . o
C)
Answer _____________________________
6.
13.376 kJ of heat are added to a 400.0 gram sample of water initially at 4.0
o
C. Calculate the final temperature of the water sample. Be careful with units! (Heat Capacity (C) for H
2
O is 4180 J/kg . o
C)
Answer ____________________________
Chemistry 11—Course Review
Page 5
Chemistry 11
Course Review
Unit 3—
Stoichiometry
1.
Given the following balanced equation, answer the questions following it:
2NF
3(g)
+ 3H
2(g)
N
2(g)
+ 6HF
(g)
a)
If 5.5 moles of H
2
are reacted, how many moles of NF
3
will be consumed? Answer ____________
b)
In order to produce 0.47 moles of HF, how many moles of NF
3
would be consumed? Answer ____________
c)
If you needed to produce 180.6 g of N
2
, how many moles of H
2
would you need to start with? Answer ____________
d)
If you completely react 17.04 g of NF
3
, what mass of HF will be produced? Answer ____________
2.
Given the following balanced equation, answer the questions following it:
HBrO
3
+ 5 HBr
3 H
2
O
(l)
+ 3 Br
2(g)
a)
If 3.56 moles of HBr are reacted, how many litres of Br
2
will be formed at STP?
Answer ______________________
Chemistry 11—Course Review
Page 6
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Chemistry 11
Course Review
HBrO
3
+ 5 HBr
3 H
2
O
(l)
+ 3 Br
2(g)
b)
In order to produce 3.311 x 10
24
molecules of Br
2
, what mass of HBr is needed?
Answer ______________________
3.
Given the following balanced chemical equation, answer the question below it.
MgCO
3 (s) + 2HCl (aq)
CO
2
(g)
+ H
2
O (l) + MgCl
2(aq)
a)
What mass of MgCO
3
will react completely with 15.0 mL of 1.5 M HCl? Answer _______________________
b)
Calculate the volume of 2.0 M HCl which would be needed to react completely with 37.935 grams of magnesium carbonate. Answer _______________________
4.
Given the following balanced equation, answer the questions below it.
Ba(OH)
2(aq)
+ 2 HNO
3(aq)
2 H
2
O
(l)
+ Ba(NO
3
)
2 a)
In an acid base reaction, 18.20 mL of 0.300 M Ba(OH)
2
is required to react completely with a 25.0 mL sample of a solution of HNO
3
. Find the [HNO
3
]. Answer _______________________
Chemistry 11—Course Review
Page 7
Chemistry 11
Course Review
b)
In an acid-base reaction, 11.06 mL of 0.200 M HNO
3 is required to react completely with a sample of 0.250 M Ba(OH)
2
. Find the volume of the Ba(OH)
2
sample. Answer _______________________
5.
Given the following balanced equation, answer the questions below it.
3 Cu
(s)
+ 8HNO
3(l)
3 Cu(NO
3
)
2(aq)
+ 2NO
(g)
+ 4 H
2
O
(l)
a)
If 317.5 grams of Cu are placed into 756.0 grams of HNO
3
, determine which reactant
is in excess. Answer _______________________
b)
If the reaction in (a) is carried out, what mass of NO will be formed? Answer _______________________
6.
Given the balanced equation: 2BN + 3F
2
2BF
3
+ N
2
,
When 161.2 grams of BN are added to an excess of F
2
, a reaction occurs in which 326.118 grams of BF
3
are formed. a)
Calculate the theoretical
yield of BF
3
in grams. Answer _______________________
b)
Calculate the percentage
yield of BF
3
. Answer _______________________
Chemistry 11—Course Review
Page 8
Chemistry 11
Course Review
7.
When reacting NH
3
with O
2
according to the reaction:
4 NH
3
+ 5 O
2
4 NO + 6 H
2
O
Using 163.2 grams of NH
3
with an excess of O
2
produces a 67% yield of NO. a)
Calculate the theoretical yield
of NO in grams. Answer _______________________
b)
Calculate the actual yield
of NO in grams. Answer _______________________
Unit 4—
Atoms, Periodic Table and Bonding
1.
The Greek who developed the idea of atoms was _______________________________
2.
Consider the following ideas:
Compounds are made up of molecules which are combinations of atoms
All atoms of an element are the same
Atoms of different elements are different
Atoms are indivisible particles
Who came up with these ideas? ______________________ He called the ideas, the
___________________________ Theory.
3.
___________________________ measured the charge/mass ratio of an electron and came up with the so-
called “plum pudding” model of the atom.
4.
___________________________ devised the Scattering Experiment, which showed that all atoms had a small dense __________________________.
5.
Bohr came up with an atomic model to explain the spectrum of ______________________.
He said that the atom has certain _______________ levels which are allowed. These levels corresponded to ____________________ in which electrons move. If an electron absorbs a certain amount of energy, it will jump to a ___________________ level. It will release this energy (in the form of __________________) when it falls back to a ______________ level.
What were two limitations of Bohr’s atomic model?
Chemistry 11—Course Review
Page 9
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Chemistry 11
Course Review
6.
Give the number of protons, neutrons and electrons in the following:
Isotope
Protons
Neutrons
Electrons
194
Ir
3+
202
Hg
2+
125
Te
2-
263
Sg
2
H
+
7.
Give the nuclear notation of the following:
Isotope
Protons
Neutrons
Electrons
105
157
103
51
72
48
33
42
36
54
79
54
94
150
91
8.
Element “X” is composed of the following naturally occurring isotopes:
Isotope
% Abundance
79
X
50.69
81
X
49.31
Calculate the average atomic mass of element “X” to 3 decimal places.
Element “X” is actually the real element ________________________________.
9.
Regions in space occupied by electrons are called ___________________________
10.
The principal quantum number is given the letter ____ and refers to the _______________
level.
Chemistry 11—Course Review
Page 10
Chemistry 11
Course Review
11.
Write the ground state electron configurations (eg. 1s
2
2s
2
2p
6
) for the following atoms or ions. You may use the core notation.
a)
P
b)
Mo
c)
Se
d)
Rb
e)
Cl
-
f)
Al
3+
g)
K
+
h)
S
2-
12.
In order to become stable,
an atom of Sr will __________ ___ electrons and become the ion ________
an atom of As will __________ ___ electrons and become the ion ________
an atom of Al will __________ ___ electrons and become the ion ________
an atom of Se will __________ ___ electrons and become the ion ________
an atom of N will __________ ___ electrons and become the ion ________
an atom of I will __________ ___ electrons and become the ion ________
an atom of Cs will __________ ___ electrons and become the ion ________
an atom of Te will __________ ___ electrons and become the ion ________
13.
Circle the metalloid: Be Rb Os Ge Pb Al
14.
Circle the most reactive element in the following: Na Mg Si Al Ar
15.
Circle the most reactive element in the following: Na K Rb Cs Li
16.
Circle the most reactive element in the following: Cl Br I At Ne
17.
Circle the element with the largest atomic radius of these: Na Mg Si Al Ar
18.
Circle the element with the largest atomic radius of these: N P As Sb Bi
Chemistry 11—Course Review
Page 11
Chemistry 11
Course Review
19.
Circle the element with the largest ionization energy of these: K Ca Ga As Kr
20.
Circle the element with the largest ionization energy of these: C Si Ge Sn Pb
21.
What is meant by ionization energy?
22.
Circle the element with the largest density of these: C Si Ge Sn Pb 23.
Circle the element with the largest density of these: Na K Rb Cs Li
24.
Circle the element with the highest electronegativity of these: Mg Sr Ba Ra
25.
Circle the element with the highest electronegativity of these: Mg Si S Cl
26.
Circle the element with the highest electronegativity of these: F Cl Br I
27.
What is meant by electronegativity?
28.
Circle the most metallic element of these: Be Mg Ca Sr Ba
29.
Circle the most metallic element of these: B Al Ga In Tl
30.
Circle the most metallic element of these: Ga Ge Se Br Kr
31.
Write a balanced equation for the reaction of potassium with water.
32.
Write a balanced equation for the reaction of aluminum with bromine.
33.
In an ionic bond, electrons are a.
shared equally by two atoms
b.
shared unequally by two atoms
c.
transferred from a metal to a non-metal
d.
transferred from a non-metal to a metal
e.
closer to one end of a molecule, forming a temporary dipole 34.
In a covalent bond, electrons are a.
shared equally by two atoms
b.
shared unequally by two atoms
c.
transferred from a metal to a non-metal
d.
transferred from a non-metal to a metal
e.
closer to one end of a molecule, forming a temporary dipole 35.
In a polar covalent bond, electrons are a.
shared equally by two atoms
b.
shared unequally by two atoms
c.
transferred from a metal to a non-metal
d.
transferred from a non-metal to a metal
e.
closer to one end of a molecule, forming a temporary dipole Chemistry 11—Course Review
Page 12
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Chemistry 11
Course Review
36.
In London forces, electrons are a.
shared equally by two atoms
b.
shared unequally by two atoms
c.
transferred from a metal to a non-metal
d.
transferred from a non-metal to a metal
e.
closer to one end of a molecule, forming a temporary dipole 37.
Complete the following table for shapes, polarities and intermolecular forces.
Formula
Electron
Count
General
Formula
AX
s
E
t
Molecule Shape
Bond
Angle(s)
Polarity
(Y/N)
Intermolecular
Forces
H
2
O
C
F
4
P
Cl
3
Br
2
As
F
5
Te
F
4
B
H
3
Kr
F
2
Si
H
3
Cl
C
S
2
HI
N
H
3
Chemistry 11—Course Review
Page 13
Chemistry 11
Course Review
38. Compare BeH
2
to H
2
O
a)
Lewis Dot Structures
b)
Molecular Geometry (Shapes)
c)
Bond Angle
d)
Dipole Moment (Overall Molecular Polarity)
e)
Intermolecular Forces
f)
Boiling or Freezing Point
39. Atomic vs. Ionic Radii
a)
Metal Atom vs. Metal Ion (Ca vs. Ca
2+
)
b)
Non-metal Atom vs. Non-metal Ion (Cl vs. Cl
-1
)
40. Using nuclear forces and atomic structure, explain the trend in
a)
Ionization energy across any period
b)
Electronegativity down any family
Chemistry 11—Course Review
Page 14
Chemistry 11
Course Review
Unit 4—
Solution Chemistry
Dissociation Equations
41. Write dissociation equations for the salts listed below when they are dissolved in water:
NiCl
3(
s
)
→
Ba(NO
3
)
2(
s
)
→
Li
2
CrO
4(
s
)
→
Al
2
(SO
3
)
3(
s
)
→
Rb
2
Cr
2
O
7(
s
)
→
Co(NO
2
)
2(
s
)
→
Dilution Calculations
M
1
V
1
= M
2
V
2
42. A student dilutes 90.0 mL of 1.25 M
lithium sulphate solution by adding 150.0 mL of water to it. Calculate the molarity of the Li
2
SO
4
and also the Li
+1
(
aq
)
.
43. During a lab activity a student heats a beaker containing 140.0 mL of 0.340 M
CuCl
2
until the volume of
the solution is reduced by 25.0 mL. Calculate the molarity of the resulting solution.
44. When equal volumes of the following 0.20 M solutions are combined, determine if a reaction results in the formation of a precipitate. If a precipitate forms write a balanced chemical equation, a complete ionic equation and a net ionic equation.
a) KCl + AgNO
3
b) SnCl
2
+ Na
3
PO
4
c) FeBr
3
+ LiOH
45. Identify the spectator ions in each of the equations in question 44.
Chemistry 11—Course Review
Page 15
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
Related Documents
Related Questions
Basic Analytical Chemistry
arrow_forward
Part D-Yield Calculations
Which of the following errors could cause your percent yield to be falsely high, or even over 100%?
Select ALL that apply.
Taking the mass of all samples with the lid included.
Handling the crucible directly with your hands.
Taking the mass of the empty crucible without the lid, but including the lid in all other mass measurements.
Heating the sample too vigorously.
Failing to completely decompose the sodium bicarbonate sample.
Submit Previous Answers Request Answer
X Incorrect; Try Again; One attempt remaining
Provide Feedback
arrow_forward
Br
Br
2.
1. Mg.
Et₂0 3. H3O+
1. Mg
Et₂O
1. Mg
Et₂0
2.
3. H3O+
Дон
2.
H
3. H3O+
CH3
/Et₂0
0/E1₂0
Et₂0
arrow_forward
please answer this question in the same format that's in the picture below. (Example picture.) answer correctly.Question: Calculate the mass in grams for: 0.75 mol hydrogen sulfide (H2S).
arrow_forward
sity o...
Fingsbo...
ckboard...
EARED4
Method? 7...
9
2
W
6
9
QUESTION 5
One mole of copper(II) sulfate, CuSO4, contains
2.41 x 1023
2.41 x 1024
6.02 x 1023
1.51 x 1023
4
Click Save and Submit to save and submit. Click Save All Answers to save all answers.
3
16
MAF 1
23
H
R
T
moles of O.
tv
Y
8
Save All Answers
8
0.22
S
arrow_forward
105 g of MgCl2 contains ________ mol MgCl2.
Group of answer choices
1.76
1.10
1.06 x 1024
6.62 x 1023
105
arrow_forward
Types of Chemical Reactions: Double Replacement
__BaCl,
_K₂SO4
a) Bak₂ + CISO4
b)
BaSO4 + KCL
c)
Ba₂SO4 + K₂Cl₂
d) BaSO4 + K₂Cl
+
_CaCl₂ +
a) CaSO4 + K₂Cl₂
b) Cak₂ + CISO4
c) CaSO4 + KCI
d) Ca(SO4)2 + K₂Cl
K₂SO4 →
+
+
_AgNO3 + _Na₂CO3 →
a) Ag₂CO3 + NaNO3
Ag₂CO3 + Na₂NO3
b)
c) Ag₂CO3 + Na(NO3)2
d) AgNa + NO₂CO3
_AgNO3 + NaCl →
a) AgCl + NaNO3
b)
Ag₂Cl + Na₂NO3
c)
Ag₂Cl +
d) AgNa+ NO3Cl
Na(NO3)2
+
arrow_forward
1. Convert 95.21 g of MgCl to mole.
2. Convert 13.18 g of AIF to mole.
3. Convert 4 moles of C6H12O6 to grams.
4. Convert 23 moles of O2 to grams.
5. Find the molar mass of C6H10O5.
arrow_forward
CaCl2 + Na2CO3 --->
Given 74.3 g of CaCl2 and 5.94 x 1023 formula units of Na2CO3 , how may formula units of NaCl would be formed? If 70.5 g of NaCl is collected during lab, what is the percent yield of NaCl in the reaction?
________ x10^_________ formula units NaCl
________ % NaCl
Blank 1:
Blank 2:
Blank 3:
arrow_forward
Determine the mass in grams of 1.6 x 10-3 mol glucose, CsH12O6
TARTING AMOUNT
ADD FACTOR
ANSWER
RESET
*( )
%3D
6.022 x 1023
12.01
0.29
180.18
0.13
9.6 x 1020
1
1.6 x 10-3
84.18
g C6H12O6
mol CoH12Oe
g CeH12O6/mol
molecules CH½O6
arrow_forward
Please help with questions 1-4
arrow_forward
Please help me with this problem using the number in the boxes thanks
arrow_forward
Give complete answers to all pre-lab questions in your laboratory notebook. (The reader should be able
to interpret the answer without referring to the lab.)
For numerical calculations, show all work with units in each step. Report final values to correct sig figs
with correct units.
1. Explain the difference between equivalence points and end point.
2. Write the chemical formula of acetic acid and then calculate its molar mass.
3. Write the balanced chemical equation between acetic acid and sodium hydroxide solution.
Include states for all reactants and products.
4. How many milliliters of 1.50 M NaOH are required to prepare 500.0 mL of 0.785 M NaOH
solution? State the dilution equation and show all related work.
5. Our primary standard is potassium hydrogen phthalate. This is abbreviated as KHP, which is
NOT its formula.
a.
Write the chemical formula of KHP and calculate its molar mass.
b. Calculate the molarity of sodium hydroxide solution if 31.45 mL are needed to titrate 0.6570
g…
arrow_forward
Please show the work on notebook papers. 1,2,3,4 Part. Chemistry
arrow_forward
PLEASE AS SOON AS POSSIBLE!!
arrow_forward
Only calculation but all.
arrow_forward
SHOW ALL CALCULATIONS.
Mass of calcium phosphate sample
plus weigling paper
2. 332 4
0.1849
Mass of weighing paper
2.332g-0.184g= 2.148 g
Mass of calcium phosphate sample
Ca3(Po4)2
40.08(3)+[30.97+16.00(4)]2=
310.18 g/mol
Molar mass of calcium phosphate
Number of moles of calcium phosphate 2.148 g x 1mole/310.18 g/mol= 0.006925 = 7.025 x 10°
in your sample
Moles of phosphorus in your sample
Mass of phosphorus in your sample
Percent phosphorus in your sample
Percent of phosphorous in one mole
of calcium phosphate
arrow_forward
I'd just like to know if question 3c's answer is correct, please and thank you.
arrow_forward
Calculate the number of moles in the following quantities:
| Correct.
1.94 g NaHCO3
0.0230
mol
the tolerance is +/-5%
SHOW HINT SHOW SOLUTION
|Incorrect. Does the answer have the appropriate units? Did you convert to g?
559 mg ZnCl2
mol
the tolerance is +/-5%
X Incorrect. Did you multiply or divide by Avogadro's number?
9.5 x 1024 molecules CO2
mol
arrow_forward
please answer these two questions will mark as helpful
arrow_forward
|||
Initial Knowledge Check
Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients.
Br₂ (1) + 1₂ (s)
IBr; (g)
Question 4
X
arrow_forward
This is a lab experiment on Stoichiometry. I am struggling with questions 2b, 2c, 2d? I attached the photo.
arrow_forward
Pressure
Volume
Temperature
(K)
Sample
Substance
(atm)
(L)
A.
02
600
1
2.
B.
Kr
273
1.
C.
Xe
273
Which 2 substances have the same number of moles?
2.
arrow_forward
I am needing help on 3 please. Thank you!
arrow_forward
Please help with question 1
arrow_forward
I Review | Constants | Periodic Table
When 55.3 g of calcium is reacted with nitrogen gas, 27.6 g of calcium nitride is produced.
Part A
What is the percent yield of calcium nitride for this reaction?
3Ca(s) + N2 (g)→Cag N2 (s)
Express your answer with the appropriate units.
HẢ
The percent yield of Ca,N2
Value
Units
Submit
Request Answer
Provide Feedback
Next >
arrow_forward
EXPERIMENT : GRAVIMETRIC ANALYSIS OF PHOSPHORUS IN PLANT FOOD
Aim: To determine the amount of phosphorus in a commercial plant food
I want the Calculations for this experiment
arrow_forward
Please answer 2d,2e,2f
arrow_forward
%30&daunchu
h 3, 31-36
3 attempts left
Check my work
Be sure to answer all parts.
The density of water is 1.00 g/mL at 4°C. How many water molecules are present in 2.46 mL of water at
this temperature?
x 10
molecules
Enter your answer in scientific notation.
< Prev
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Related Questions
- Basic Analytical Chemistryarrow_forwardPart D-Yield Calculations Which of the following errors could cause your percent yield to be falsely high, or even over 100%? Select ALL that apply. Taking the mass of all samples with the lid included. Handling the crucible directly with your hands. Taking the mass of the empty crucible without the lid, but including the lid in all other mass measurements. Heating the sample too vigorously. Failing to completely decompose the sodium bicarbonate sample. Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining Provide Feedbackarrow_forwardBr Br 2. 1. Mg. Et₂0 3. H3O+ 1. Mg Et₂O 1. Mg Et₂0 2. 3. H3O+ Дон 2. H 3. H3O+ CH3 /Et₂0 0/E1₂0 Et₂0arrow_forward
- please answer this question in the same format that's in the picture below. (Example picture.) answer correctly.Question: Calculate the mass in grams for: 0.75 mol hydrogen sulfide (H2S).arrow_forwardsity o... Fingsbo... ckboard... EARED4 Method? 7... 9 2 W 6 9 QUESTION 5 One mole of copper(II) sulfate, CuSO4, contains 2.41 x 1023 2.41 x 1024 6.02 x 1023 1.51 x 1023 4 Click Save and Submit to save and submit. Click Save All Answers to save all answers. 3 16 MAF 1 23 H R T moles of O. tv Y 8 Save All Answers 8 0.22 Sarrow_forward105 g of MgCl2 contains ________ mol MgCl2. Group of answer choices 1.76 1.10 1.06 x 1024 6.62 x 1023 105arrow_forward
- Types of Chemical Reactions: Double Replacement __BaCl, _K₂SO4 a) Bak₂ + CISO4 b) BaSO4 + KCL c) Ba₂SO4 + K₂Cl₂ d) BaSO4 + K₂Cl + _CaCl₂ + a) CaSO4 + K₂Cl₂ b) Cak₂ + CISO4 c) CaSO4 + KCI d) Ca(SO4)2 + K₂Cl K₂SO4 → + + _AgNO3 + _Na₂CO3 → a) Ag₂CO3 + NaNO3 Ag₂CO3 + Na₂NO3 b) c) Ag₂CO3 + Na(NO3)2 d) AgNa + NO₂CO3 _AgNO3 + NaCl → a) AgCl + NaNO3 b) Ag₂Cl + Na₂NO3 c) Ag₂Cl + d) AgNa+ NO3Cl Na(NO3)2 +arrow_forward1. Convert 95.21 g of MgCl to mole. 2. Convert 13.18 g of AIF to mole. 3. Convert 4 moles of C6H12O6 to grams. 4. Convert 23 moles of O2 to grams. 5. Find the molar mass of C6H10O5.arrow_forwardCaCl2 + Na2CO3 ---> Given 74.3 g of CaCl2 and 5.94 x 1023 formula units of Na2CO3 , how may formula units of NaCl would be formed? If 70.5 g of NaCl is collected during lab, what is the percent yield of NaCl in the reaction? ________ x10^_________ formula units NaCl ________ % NaCl Blank 1: Blank 2: Blank 3:arrow_forward
- Determine the mass in grams of 1.6 x 10-3 mol glucose, CsH12O6 TARTING AMOUNT ADD FACTOR ANSWER RESET *( ) %3D 6.022 x 1023 12.01 0.29 180.18 0.13 9.6 x 1020 1 1.6 x 10-3 84.18 g C6H12O6 mol CoH12Oe g CeH12O6/mol molecules CH½O6arrow_forwardPlease help with questions 1-4arrow_forwardPlease help me with this problem using the number in the boxes thanksarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning