Pearson eText Basic Chemistry -- Instant Access (Pearson+)
6th Edition
ISBN: 9780135765982
Author: Karen Timberlake, William Timberlake
Publisher: PEARSON+
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Textbook Question
Chapter 13, Problem 62APP
For each of the following reactions, indicate if the equilibrium mixture contains mostly products, mostly reactants, or both reactants and products:
a.
b.
c.
d.
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Consider the following reaction:
2SO3 (g)2SO2(g) + 02 (9)
If 0.0942 moles of
SO3(g), 0.426 moles of
SO2, and 0.310 moles of
O2 are at equilibrium in a 17.4 L container at 1320 K, the value of the equilibrium constant,
Kc, is
(14a) The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K.2CH2Cl2(g) CH4(g) + CCl4(g) Calculate the equilibrium concentrations of reactant and products when 0.382 moles of CH2Cl2 are introduced into a 1.00 L vessel at 350 K.
[CH2Cl2]
= ___
M
[CH4]
= ___
M
[CCl4]
= ____
M
(b) The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K.CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.271 moles of CO and 0.271 moles of Cl2 are introduced into a 1.00 L vessel at 600 K.
[CO]
= ____
M
[Cl2]
= _____
M
[COCl2]
= _____
M
Consider the following system at equilibrium where AHⓇ
2SO2(g) + O2(g) = 2SO3 (9)
When 0.24 moles of O₂ (g) are added to the equilibrium system at constant temperature:
The value of K
O increases
decreases
O remains the same
The value of Qc
O is greater than Kc
O is equal to Kc
O is less than Kc
=
198 kJ, and Ke
The concentration of SO2 will
O increase
decrease
O remain the same
The reaction must
O run in the forward direction to reestablish equilibrium
O run in the reverse direction to reestablish equilibrium
O remain in the current position, since it is already at equilibrium
=
34.5, at 1150 K:
Consider the following mat equilibrium where&ff-879
PC)+)-PC, (
Whe036PC (a) are added to the equum system at
The K
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Chapter 13 Solutions
Pearson eText Basic Chemistry -- Instant Access (Pearson+)
Ch. 13.1 - Prob. 1PPCh. 13.1 - Prob. 2PPCh. 13.1 - In the following reaction, what happens to the...Ch. 13.1 - Prob. 4PPCh. 13.1 - Prob. 5PPCh. 13.1 - Prob. 6PPCh. 13.2 - What is meant by the term reversible reaction?Ch. 13.2 - Prob. 8PPCh. 13.2 - Which of the following are at equilibrium? a. The...Ch. 13.2 - Which of the following are not at equilibrium? a....
Ch. 13.2 - 13.11 The following diagrams show the chemical...Ch. 13.2 - Prob. 12PPCh. 13.3 - Write the equilibrium expression for each of the...Ch. 13.3 - Prob. 14PPCh. 13.3 - Prob. 15PPCh. 13.3 - Prob. 16PPCh. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - What is the numerical value of Kc for the...Ch. 13.3 - Prob. 21PPCh. 13.3 - Identify each of the following as a homogeneous or...Ch. 13.3 - Prob. 23PPCh. 13.3 - Prob. 24PPCh. 13.3 - Prob. 25PPCh. 13.3 - What is the numerical value of Kc for the...Ch. 13.4 - Prob. 27PPCh. 13.4 - Prob. 28PPCh. 13.4 - Indicate whether each of the following equilibrium...Ch. 13.4 - Indicale whether each of the following equilibrium...Ch. 13.4 - Prob. 31PPCh. 13.4 - The numerical value of the equilibrium constant,...Ch. 13.4 - Prob. 33PPCh. 13.4 - The numerical value of the equilibrium constant,...Ch. 13.5 - In the lower atmosphere, oxygen is converted to...Ch. 13.5 - Prob. 36PPCh. 13.5 - Hydrogen chloride can be made by reacting hydrogen...Ch. 13.5 - When heated, carbon monoxide reacts with water to...Ch. 13.5 - Use the following equation for the equilibrium of...Ch. 13.5 - Use the following equation for the equilibrium of...Ch. 13.5 - Prob. 41PPCh. 13.5 - Prob. 42PPCh. 13.6 - For each of the following slightly soluble ionic...Ch. 13.6 - For each of the following slightly soluble ionic...Ch. 13.6 - Prob. 45PPCh. 13.6 - Prob. 46PPCh. 13.6 - A saturated solution of silver carbonate, Ag2CO3 ,...Ch. 13.6 - Prob. 48PPCh. 13.6 - Calculate the molar solubility, S , of CuI if it...Ch. 13.6 - Calculate the molar solubility, S , of SnS if it...Ch. 13.6 - The CO2 level in the atmosphere has increased over...Ch. 13.6 - Prob. 52PPCh. 13 - Write the equilibrium expression for each of the...Ch. 13 - Write the equilibrium expression for each of the...Ch. 13 - Prob. 55UTCCh. 13 - Would the equilibrium constant, Ke , for the...Ch. 13 - Prob. 57UTCCh. 13 - Prob. 58UTCCh. 13 - Prob. 59APPCh. 13 - Prob. 60APPCh. 13 - For each of the following reactions, indicate if...Ch. 13 - For each of the following reactions, indicate if...Ch. 13 - Consider the reaction: (13.3) 2NH3(g)N2(g)+3H2(g)...Ch. 13 - Prob. 64APPCh. 13 - Prob. 65APPCh. 13 - Prob. 66APPCh. 13 - Prob. 67APPCh. 13 - According to Le Châtelier's principle, does the...Ch. 13 - Prob. 69APPCh. 13 - Prob. 70APPCh. 13 - The numerical value of the equilibrium constant,...Ch. 13 - The numerical value of the equilibrium constant,...Ch. 13 - For each of the following slightly soluble ionic...Ch. 13 - For each of the following slightly soluble ionic...Ch. 13 - Prob. 75APPCh. 13 - Prob. 76APPCh. 13 - Prob. 77APPCh. 13 - Prob. 78APPCh. 13 - What is the molar solubility, S , of CdS if it has...Ch. 13 - Prob. 80APPCh. 13 - Prob. 81CPCh. 13 - Prob. 82CPCh. 13 - Prob. 83CPCh. 13 - Indicate how each of the following will affect the...Ch. 13 - Prob. 85CPCh. 13 - Prob. 86CPCh. 13 - Prob. 87CPCh. 13 - Prob. 88CP
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- The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.arrow_forwardMustard gas, used in chemical warfare in World War I, has been found to be an effective agent in the chemotherapy of Hodgkin's disease. It can be produced according to the following reaction: SCl2(g)+2C2H4(g)S(CH2CH2Cl)2(g)An evacuated 5.0-1- flask at 20.0C is filled with 0.258 mol SCl2 and 0.592 mol C2H4. After equilibrium is established, 0.0349 mol mustard gas is present. (a) What is the partial pressure of each gas at equilibrium? (b) What is K at 20.0C?arrow_forward. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO 2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?arrow_forward
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- At a certain temperature, Kc = 0.18 for the following reaction:PCl3 (g) + Cl2 (g) PCl5 (g)Suppose a reaction vessel at this temperature contained these three gases at the following concentrations:[PCl3] = 0.420 M, [Cl2] = 0.240 M, [PCl5] = 0.00500 M:(10a): Is the system in a state of equilibrium? Justify your answer with a calculation.(10b): If the system is not in equilibrium, which direction will the reaction proceed to reach equilibrium?arrow_forward9 Methanol is produced synthetically: CO (g) + 2H2 (g) CH;OH (g) A H=+24 Kcal a) Write the Equilibrium Constant Expression: b) Is it an Endothermic or Exothermic Reaction? c). Indicate the effect on the equilibrium, ie., does the reaction shift to the right, to the left, or have no effect on the reaction at all: 1. Increase in [2H2] = 2. Decrease in [CO] = 3. Increase in Temperature = 4. Increasc in Pressure = 5. Addition of a catalyst =,arrow_forwardCarbon dioxide and water react to form methanol and oxygen, like this: 2 CO₂(g) + 4H₂O(g) 2 CH₂OH(1)+3 0₂(g) At a certain temperature, a chemist finds that a 7.5 L reaction vessel containing a mixture of carbon dioxide, water, methanol, and oxygen at equilibrium has the following composition: compound amount CO₂ 3.25 g H₂O 2.85 g CH3OH 3.00 g 0₂ 1.83 g Calculate the value of the equilibrium constant K for this reaction. Round your answer to 2 significant digits. = 0 x10arrow_forward
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