EP BASIC CHEMISTRY-MODIFIED MASTERING
6th Edition
ISBN: 9780137452392
Author: Timberlake
Publisher: SAVVAS L
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Chapter 10, Problem 110CP
An ice cube at 0 °C with a mass of 115 g is added to water in a beaker that has a temperature of 64.0 °C. If the final temperature of the mixture is 24.0 °C, what was the initial mass of the warm water? (10.7)
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Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NOCI (g) 2NO (g) + Cl2 (g) AGº =41. kJ
Now suppose a reaction vessel is filled with 4.50 atm of nitrosyl chloride (NOCI) and 6.38 atm of chlorine (C12) at 212. °C. Answer the following questions
about this system:
?
rise
Under these conditions, will the pressure of NOCI tend to rise or fall?
x10
fall
Is it possible to reverse this tendency by adding NO?
In other words, if you said the pressure of NOCI will tend to rise, can that
be changed to a tendency to fall by adding NO? Similarly, if you said the
pressure of NOCI will tend to fall, can that be changed to a tendency to
rise by adding NO?
yes
no
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of NO needed to reverse it.
Round your answer to 2 significant digits.
0.035 atm
✓
G
00.
18
Ar
Highlight each glycosidic bond in the molecule below. Then answer the questions in the table under the drawing area.
HO-
HO-
-0
OH
OH
HO
NG
HO-
HO-
OH
OH
OH
OH
NG
OH
€
+
Suppose the molecule in the drawing area below were reacted with H₂ over a platinum catalyst. Edit the molecule to show what would happen to it. That is, turn
it into the product of the reaction.
Also, write the name of the product molecule under the drawing area.
Name: ☐
H
C=0
X
H-
OH
HO-
H
HO-
-H
CH₂OH
×
Chapter 10 Solutions
EP BASIC CHEMISTRY-MODIFIED MASTERING
Ch. 10.1 - Determine the total number of valence electrons...Ch. 10.1 - Determine the total number of valence electrons...Ch. 10.1 - Prob. 3PPCh. 10.1 - If the available number of valence electrons for a...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.1 - Draw the Lewis structures for each of the...Ch. 10.2 - Prob. 9PPCh. 10.2 - When does a molecular compound have resonance?
Ch. 10.2 - Draw two resonance structures for each of the...Ch. 10.2 - Draw two resonance structures for each of the...Ch. 10.3 - Prob. 13PPCh. 10.3 - Choose the shape (1 to 6) that matches each of the...Ch. 10.3 - Prob. 15PPCh. 10.3 - Prob. 16PPCh. 10.3 - Prob. 17PPCh. 10.3 - Prob. 18PPCh. 10.3 - Use VSEPR theory to predict the shape of each of...Ch. 10.3 - Prob. 20PPCh. 10.3 - Prob. 21PPCh. 10.3 - Draw the Lewis structure and predict the shape for...Ch. 10.4 - Describe the trend in electronegativity as...Ch. 10.4 - Describe the trend in electronegativity as...Ch. 10.4 - Prob. 25PPCh. 10.4 - Which electronegativity difference (a, b, or c)...Ch. 10.4 - Using the periodic table, arrange the atoms in...Ch. 10.4 - Using the periodic table, arrange the atoms in...Ch. 10.4 - Predict whether the bond between each of the...Ch. 10.4 - Predict whether the bond between each of the...Ch. 10.4 - For the bond between each of the following pairs...Ch. 10.4 - For the bond between each of the following pairs...Ch. 10.5 - Why is F2 a nonpolar molecule, but HF is a polar...Ch. 10.5 - Why is CCl4 a nonpolar molecule, but PCl3 is a...Ch. 10.5 - Identify each of the following molecules as polar...Ch. 10.5 - Identify each of the following molecules as polar...Ch. 10.5 - Prob. 37PPCh. 10.5 - Prob. 38PPCh. 10.6 - Prob. 39PPCh. 10.6 - Prob. 40PPCh. 10.6 - Identify the strongest intermolecular forces...Ch. 10.6 - Identify the strongest intermolecular forces...Ch. 10.6 - Prob. 43PPCh. 10.6 - Prob. 44PPCh. 10.7 - Using Figure 10.6, calculate the heat change...Ch. 10.7 - Using Figure 10.6, calculate the heat change...Ch. 10.7 - Prob. 47PPCh. 10.7 - Using Figure 10.6, calculate the heat change...Ch. 10.7 - Using Figure 10.6 and the specific heat of water,...Ch. 10.7 - Using Figure 10.6 and the specific heat of water,...Ch. 10.7 - An ice bag containing 275 g of ice at 0 °C was...Ch. 10.7 - Prob. 52PPCh. 10.7 - Prob. 53PPCh. 10.7 - In the preparation of liquid nitrogen, how many...Ch. 10.7 - Using the electronegativity values in Figure 10.2,...Ch. 10.7 - Prob. 56PPCh. 10.7 - Prob. 57PPCh. 10.7 - a. Draw two resonance structures for bicarbonate...Ch. 10 - State the number of valence electrons, bonding...Ch. 10 - State the number of valence electrons, bonding...Ch. 10 - Prob. 61UTCCh. 10 - Prob. 62UTCCh. 10 - Consider the following bonds: Ca and O, C and O, K...Ch. 10 - Consider the following bonds: F and Cl, Cl and Cl,...Ch. 10 - Identify the major intermolecular forces between...Ch. 10 - Prob. 66UTCCh. 10 - Prob. 67UTCCh. 10 - Prob. 68UTCCh. 10 - Prob. 69UTCCh. 10 - Prob. 70UTCCh. 10 - Prob. 71UTCCh. 10 - Prob. 72UTCCh. 10 - Prob. 73APPCh. 10 - Determine the total number of valence electrons in...Ch. 10 - Draw the Lewis structures for each of the...Ch. 10 - Draw the Lewis structures for each of the...Ch. 10 - Draw resonance structures for each of the...Ch. 10 - Prob. 78APPCh. 10 - Use the periodic table to arrange the following...Ch. 10 - Use the periodic table to arrange the following...Ch. 10 - Select the more polar bond in each of the...Ch. 10 - Select the more polar bond in each of the...Ch. 10 - Show the dipole arrow for each of the following...Ch. 10 - Show the dipole arrow for each of the following...Ch. 10 - Calculate the electronegativity difference and...Ch. 10 - Calculate the electronegativity difference and...Ch. 10 - Prob. 87APPCh. 10 - For each of the following, draw the Lewis...Ch. 10 - For each of the following, draw the Lewis...Ch. 10 - For each of the following, draw the Lewis...Ch. 10 - Prob. 91APPCh. 10 - Predict the shape and polarity of each of the...Ch. 10 - Prob. 93APPCh. 10 - Prob. 94APPCh. 10 - Prob. 95APPCh. 10 - Indicate the major type of intermolecular...Ch. 10 - When it rains or snows, the air temperature seems...Ch. 10 - Prob. 98APPCh. 10 - Using Figure 10.6, calculate the grams of ice that...Ch. 10 - Using Figure 10.6, calculate the grams of ethanol...Ch. 10 - Prob. 101APPCh. 10 - Using Figure 10.6, calculate the grams of benzene...Ch. 10 - Prob. 103CPCh. 10 - Prob. 104CPCh. 10 - Prob. 105CPCh. 10 - Prob. 106CPCh. 10 - Prob. 107CPCh. 10 - The melting point of benzene is 5.5 °C, and its...Ch. 10 - A 45.0-g piece of ice at 0.0 °C is added to a...Ch. 10 - An ice cube at 0 °C with a mass of 115 g is added...Ch. 10 - Prob. 111CPCh. 10 - Prob. 112CPCh. 10 - Prob. 13CICh. 10 - Prob. 14CICh. 10 - Prob. 15CICh. 10 - Ethanol, C2H6O , is obtained from renewable crops...Ch. 10 - Chloral hydrate, a sedative and hypnotic, was the...Ch. 10 - Ethylene glycol, C2H6O2 , used as a coolant and...Ch. 10 - Prob. 19CICh. 10 - Prob. 20CI
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