Consider the following equation: CO + 2H 2 -Calculate the amount of heat (in kJ) released when 4.58 g H2. react with 161.2 g of CO.- CH 30H AH rxn = -128 kJ11.0061314153.Li6.944.Be901226.10.811201114.00121314SI28.08515NaMgAl22.990 24.305347.9.10111226.98230.9741920KCa39.098 40.07821222325Mn51.996 54.938242627Co28Ni58.69329Cu63.54630Zn65 38313233As74.922ScTiCrFeGaGe44.95647.86750.94255.84558.93369.723726303738Sr87.6239Y-88.90640414243Te4445Rh46Pd47484950Sn118.7151Sb121.76RbZr91.224NbMoRuAg107.87In85 46892.90695.95(98)101.07102.91106.4211241114.825556Ba57-7172H73747576Os7778Pt79Au80818283CsTaReIrHg200.59PbBi208.98132.91137.33178 49180.95183.84186.21190.23192.22195.08196.97204.38207.287Fr(223)88Ra(226)89-103104105Db(268)106107Bh(270)108Hs(277)109Mt(276)IIIRg(280)110Rr(265)Sg(271)112Cn(285)113Nh(286)114FI(289)115MeDs(281)(289)• Lanthanideseries57La138.915859Pr140.9161Pm(145)6062Sm150.366364656667Но68CeNdEuGd157.25Tb158.93Dy162.50Er140.12144.24151.96164.93167.26# Actinideseries8990919293949596979899100Th 8LOOP 860644.956 47.86750.94240Zr41Nb92.90642Мо95.9543Tc(98)44Ru101.0745Rh102.9146Pd106.42383937Rb85.468 87.62Sr88.906 91.22478Pt195.08767775Re7472Hf73Ta57-7156Ba137.33Os55Cs132.91Ir180.95183.84186.21190.23192.22178.49106Sg(271)107Bh(270)108Hs(277)109Mt(276)110Ds(281)89-10387Fr(223)88Ra(226)104Rf(265)105Db(268)Lanthanideseries61Pm(145)62Sm150.3663Eu151.966057La58Ce140.1259Pr140.91Nd138.91144.2494Pu(244)95Am(243)9293# Actinideseries89Ac(227)90Th232.0491Pa231.04Np(237)238.03O -256 kJO -1024 kJO -239 kJO -1034 kJO -145 kJ

Answered: Image /qna-images/answer/69ca697c-2a19-4f8b-bc6f-07b9572f41b0.jpg

Answered: Consider the following equation: CO +…

Consider the following equation: CO + 2H 2 CH 3OH AH pm = -128 kJ Calculate the amount of heat (in kJ) released when 4.58 g H2. react with 161.2 g of CO.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: The thermochemical equation for the combustion of methanol is CH₂OH (g) + 3/2 0₂(g) → CO₂(g) + 2 H₂O…

A: To find kJ of heat, convert the given mass of methanol to moles. Then, multiply the obtained moles…

Q: Consider the following reaction: 2 Mg + O2 2 MgO, Hrxn = -1,203 kJ.Calculate the amount of heat…

A: The given balanced chemical reaction is as follows:

Q: 4.78 x 10 kJ E) 1,040 kJ 51.Methanol (CH,OH) burns according to the equation 2CH,OH(I) +…

A: The given reaction is,

Q: The specific heat capacity of silver is 0.24 J/°C·g. Calculate the energy required to raise the…

A: Heat capacity is an extensive property. But specific heat capacity is intensive property. Heat…

Q: How much heat is absorbed or released when 40.00 g of NH3(g) reacts in the presence of excess O2(g)…

A: According to the question, The mass of the ammonia gas is given by =40.00 g The molar mass of the…

Q: How much heat is rel;eased to the surroundings when 5.00g of CO2 is produced according to the…

A: .reaction given in question states that 2220 kj energy released in production of 3 moles of CO2 .…

Q: Consider the dissolution of CaCl2: CaCl2 (s) → Ca²+ (ag) +2 Cl¯(ag) AH=-81,5 kJ An 11.8-g sample of…

A: When a solute is dissolved in solvent to form a solution is called dissolution. It measures the…

Q: Given the reaction: 4 Fe(s) + 302(g) → 2 Fe203(s) A H= -1652 kJ, what is the enthalpy change when…

A: for a given reaction, 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) enthalpy change, Δ H = -1652 KJ

Q: 2 C4H10(g) + 13 O2(g) --> 8 CO2(g) + 10 H2O(l) change in H = -5756.84 kJ The enthalpy change during…

A: The objective of the question is to find out the mass of CO2 produced in a reaction with a given…

Q: רPi How much heat will be released (AH) if 0.2037 mol of NH3 are mixed with 0.20 mol of O2 in the…

Q: How much heat is rel;eased to the surroundings when 5.00 g of CO2 is produced according to the…

A: We can solve the problem by determining the moles of CO2 that is actually produced in the reaction.…

Q: How much heat will be released (AH) if 0.4391 mol of NHs are mixed with 0.20 mol of O2 in the…

A: Change in enthalpy (∆H) is proportional to the number of moles of reactants and products associated…

Q: Elemental iron is used in heat packs and the reaction can be represented as: 4 Fe(s) +3 O2(g) → 2…

A: When enthalpy is negative that means reaction is exothermic reaction

Q: How much heat is evolved when 453.5 g of ammonia (NH3) is produced according to the following…

A: Given Reaction is - N2 (g) + 3H2 (g) → 2NH3 (g) ΔH= -91.8 kJ

Q: Given the chemical reaction: CHale) +5 0,g)→3 CO,) +4 H,OG) AH = -2044 kJ How much heat would be…

A: When hydrocarbons are combusted, then the large amount of heat is produced which is known as…

Q: if 11.2 g of H2 (g) (MM = 2.016 g/mol) were to react according to the balanced equation given below,…

A: We have to calculate the heat released amount.

Q: A generic solid, X, has a molar mass of 59.1 g/mol. In a constant-pressure calorimeter, 15.8 g of X…

A: Given: The mass of solid X = 15.8 g The mass of water = 311 g The initial temperature of the water =…

Q: 17) A 22.9 g sample of iron absorbs 155 J of heat, sample upon which the temperature of the…

Q: When 4.88 g of a solid mixture composed of NH¼CI and CaCl2 was dissolved in 100.0 mL of water, the…

A: Given that : The mass of the solid mixture = 4.88 g The volume of water = 100.0 mL The rise in…

Q: AH soln %3D II

Q: a) Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H20(g) AH = -2035 kJ How much heat is…

A: Formula used :- Q = mCpdT Where m is mass , Cp is specific heat capacity and dT is change in…

Q: A 4.77 g sample of an unknown salt (MM = 116.82 g/mol) is dissolved in 150.00 g water in a coffee…

A: Given information: Mass of unknown sample = 4.77 g Mass of water = 150.00 g Initial temperature =…

Q: Liquid hydrogen peroxide is an oxidizing agent in many rocket fuel mixtures because it releases…

Q: A balanced, generic thermochemical equation is shown below. A, B, and C are substances involved in…

Q: In the following reaction, how much heat is generated when 3.21moles of CH4 are burned

A: The negative sign before ∆H0 shows that heat is released from the reaction. Observing the given…

Q: 1) Glucose, C6H12O6 (MM = 180 g/mol), is converted into ethyl alcohol, C2H5OH(l) in the fermentation…

Q: In the following reaction, how much heat is generated when 3.27 moles of CH« are burned? CH: (g) + 2…

A: The reaction is : CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) ∆H°=-802 kJ/mol Here, as we can…

Q: 2. Mercury (II) oxide is a reddish mineral that is used as the cathode in mercury batteries. It is…

A: In the above question the heat energy require to prepare 2 mole Hg have given . We have to calculate…

Q: The specific heat capacity of a pure substance can be found by dividing the heat needed to change…

Q: OWhen a 0.740-g sample of trinitrotoluene (TNT), CH-N,Oo, is bumed in a bomb calorimeter, the…

A: Given volume of water = 675mL Density of water = 1g/mL So, mass of water = volume×density = 675g…

Q: Potassium nitrate, KNO,, has a molar mass of 101.1 g/mol. In a constant-pressure calorimeter, 47.3 g…

Q: When a 6.00 g sample of KBr is dissolved in water in a calorimeter that has a total heat capacity of…

A: The question is based on the concept of specific heat capacity.It is defined as the amount of heat…

Q: Consider the reaction B2H6(g) + 3 O2(g) → B2O3(s) + 3 H₂O(g) AH = -2035 kJ/mol Calculate the amount…

Q: A calorimeter contains 16.0 mL of water at 14.5 °C. When 2.20 g of X (a substance with molar mass of…

A: Given : Mass of X = 2.20 g Volume of water = 16.0 mL Heat capacity (C) = 4.18 ∆T = 25.5 - 14.5 =…

Q: Calculate the energy produced when 5.0 mol of CO2 are produced on the basis of the following…

Q: What is the specific heat of a 74.01g piece of an unkown metal that exhibits a 45.2 Celcius…

Q: Consider the reaction. 2Fe2O3⟶4Fe+3O2. Δ?∘rxn=+824.2 kJ The formation of 12.0 g of O2…

A: 2Fe2O3 ——> 4Fe + 3O2 Heat = +824.2 kJ Clearly, this heat is released when 3 moles of O2…

Q: When a 4.00 g sample of RbBr is dissolved in water in a calorimeter that has a total heat capacity…

A: First, we will calculate the enthalpy change and then convert that heat into a molar quantity. To…

Q: 61. Consider the thermochemical equation for the combustion of acetone (C3H,O), the main ingredient…

Q: The complete combustion of propane, C 3H 8(g), is represented by the equation: C 3H 8(g) + 5 O 2(g)…

A: when the heat is evolved in a reaction then that reaction is known as exothermic reaction. The…

Q: H() + 3 O2(g) → 2 CO2(g) +4 H 452.8 kJ/mol ch heat (kJ) is evolved when 3 pl (CH3OH) with a density…

A: Volume of methanol = 35 mL Density = 0.792 g/mL Mass = Volume × density = 35 × 0.792 = 27.72 g…

Q: An experiment is carried out where 12.2g of NaOH is dissolved in 240.0g of water in a coffee cup…

A: The experiment is the measurement of heat of dissolution of NaOH.

Q: How much heat (in kJ) will be released (AH) if 1.20 mol of SrO is mixed with 0.951 mol of CO2 in the…

A: We will calculate heat in kj

Q: An experiment was performed to calculate the heat of solution for potassium fluoride. Use the…

A: Given: The mass of water=52.42 g The mass of salt sample=7.32 g The total mass of the sample,…

Question

Consider the following equation: CO + 2H 2 -
Calculate the amount of heat (in kJ) released when 4.58 g H2. react with 161.2 g of CO.
- CH 30H AH rxn = -128 kJ
1
1.006
13
14
15
3.
Li
6.94
4.
Be
90122
6.
10.81
12011
14.00
12
13
14
SI
28.085
15
Na
Mg
Al
22.990 24.305
3
4
7.
9.
10
11
12
26.982
30.974
19
20
K
Ca
39.098 40.078
21
22
23
25
Mn
51.996 54.938
24
26
27
Co
28
Ni
58.693
29
Cu
63.546
30
Zn
65 38
31
32
33
As
74.922
Sc
Ti
Cr
Fe
Ga
Ge
44.956
47.867
50.942
55.845
58.933
69.723
72630
37
38
Sr
87.62
39
Y-
88.906
40
41
42
43
Te
44
45
Rh
46
Pd
47
48
49
50
Sn
118.71
51
Sb
121.76
Rb
Zr
91.224
Nb
Mo
Ru
Ag
107.87
In
85 468
92.906
95.95
(98)
101.07
102.91
106.42
11241
114.82
55
56
Ba
57-71
72
H
73
74
75
76
Os
77
78
Pt
79
Au
80
81
82
83
Cs
Ta
Re
Ir
Hg
200.59
Pb
Bi
208.98
132.91
137.33
178 49
180.95
183.84
186.21
190.23
192.22
195.08
196.97
204.38
207.2
87
Fr
(223)
88
Ra
(226)
89-103
104
105
Db
(268)
106
107
Bh
(270)
108
Hs
(277)
109
Mt
(276)
III
Rg
(280)
110
Rr
(265)
Sg
(271)
112
Cn
(285)
113
Nh
(286)
114
FI
(289)
115
Me
Ds
(281)
(289)
• Lanthanide
series
57
La
138.91
58
59
Pr
140.91
61
Pm
(145)
60
62
Sm
150.36
63
64
65
66
67
Но
68
Ce
Nd
Eu
Gd
157.25
Tb
158.93
Dy
162.50
Er
140.12
144.24
151.96
164.93
167.26
# Actinide
series
89
90
91
92
93
94
95
96
97
98
99
100
Th

8LOOP 8606
44.956 47.867
50.942
40
Zr
41
Nb
92.906
42
Мо
95.95
43
Tc
(98)
44
Ru
101.07
45
Rh
102.91
46
Pd
106.42
38
39
37
Rb
85.468 87.62
Sr
88.906 91.224
78
Pt
195.08
76
77
75
Re
74
72
Hf
73
Ta
57-71
56
Ba
137.33
Os
55
Cs
132.91
Ir
180.95
183.84
186.21
190.23
192.22
178.49
106
Sg
(271)
107
Bh
(270)
108
Hs
(277)
109
Mt
(276)
110
Ds
(281)
89-103
87
Fr
(223)
88
Ra
(226)
104
Rf
(265)
105
Db
(268)
Lanthanide
series
61
Pm
(145)
62
Sm
150.36
63
Eu
151.96
60
57
La
58
Ce
140.12
59
Pr
140.91
Nd
138.91
144.24
94
Pu
(244)
95
Am
(243)
92
93
# Actinide
series
89
Ac
(227)
90
Th
232.04
91
Pa
231.04
Np
(237)
238.03
O -256 kJ
O -1024 kJ
O -239 kJ
O -1034 kJ
O -145 kJ

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

In the following reaction, how much heat (in kJ) is released when 6.35 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol
In the following reaction, what is the quantity of heat (in kJ) released when 3.91 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO₂ (g) + 2 H₂O(g) AH° = -802 kJ/mol -
In the following reaction, how many moles of CH;OH are required to produce -2191 kJ of heat? 2 CH;OH (I) + 3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH° = -1280. kJ mol 1 3 4 6. C 7 8 9. + +/- x 100
2. A calorimeter contains 100.0 g of water at 39.8 °C. A 12.78 g object at 100.0 ºC is placed inside the calorimeter. When equilibrium has been reached, the new temperature of the water and metal object is 40.6 °C. What is the specific heat of the metal?
A 138.9 g sample of an unknown metal at a temperature of 99.1 °C is added to 44.72 g of water at a temperature of 19.1 °C. The specific heat of water is 4.184 Jg-1 °C- 1. The final temperature of the system is 52.2°C. Calculate the specific heat of the unknown metal.
4. The reaction of 250.0 mL of a 1.00 M hydrochloric acid solution with 250.0 mL of a 1.00 M sodium hydroxide solution was carried out in a constant pressure calorimeter. The total heat capacity of the calorimeter plus solutions was 6.45 kJ/K. The temperature of the calorimeter and solutions increased by 2.11°C. What is AH (in kJ) for the neutralization of 1.00 mol HCl(aq) by NaOH(aq)? A) -54.4 B) -21.2 +12.6 +54.4 E) -12.6
NW113AACE04-21 3. a hunk of metal-like substance was found in an archeological site. In an attempt to identify it, the metal was heated and placed in a calorimeter containing water and determined the specific heat of the metal. If the specific heat of the metal is 0.448 J/g °C, what is the approximate molar mass (atomic mass) and likely identity of the metal? (Hint: compare the molar mass (atomic mass) of metal that of metals in periodic table)
Consider the following reaction carried out under constant pressure 5Cl2(g) + 2P(s) → 2PCl5(g) Δ Hrxn = -749.8 kJCalculate the heat associated with the complete reaction of 84.0 g of Cl2 with 20.6 g of P. -6.15×102 kJ -1.78×102 kJ -4.99×102 kJ -8.88×102 kJ -2.50×102 kJ
Iron has a specific heat capacity of 0.444J/g-C. 50.0 g of iron at 35C is added to 50.0 g of water with a specific heat capacity of 4.184 J/g-C. When the temperature of the resulting mixture stops changing, the temperature is closer to that of the original water than to the iron. True or false?
Octane (C8H18) is a component of gasoline that burns according to the following equation: C8H18 (l) + 25/2 O2 (g) ------> 8 CO2 (g) + 9 H2O (g) ΔHorxn = - 5074.1 kJ What mass of octane (in g) is required to produce 5830 kJ of heat?
If 100.0 gram of a metal at 100.0 oC is added to 100.0 g of water at 25.0 oC, the final temperature is 31.3 oC. What is the specific heat of the metal?
In the following reaction, how many moles of CH3OH are required to give off 3791 kJ of heat? 2 CH,OH (I) + 3 02 (g) → 2 CO, (g) + 4 H,0(g) AH° = -1280. kJ