At equilibrium, the vessel is found to contain 0.566 g of H2. (a) Calculate the equilibrium concentrations of H2, Br, and HBr. (b) Calculate Ke. На 0.1600 mol of H20 is placed in a 2.000-L vessel. The fol- lowing equilibrium is established at 500 K: CO2(8) + H2(8) = CO(g) + H2O(g) 15.37 A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and a) Calculate the initial partial pressures of CO2, H2, and H2O. = 3.51 atm. Calculate the equilib- (b) At equilibrium RH,0 rium partial pressures of CO2, H2, and CO. (c) Calculate K. for the reaction. (d) Calculate K, for the reaction. %3D 15.38 A flask is charged with 1.500 atm of N½O4(g) and 1.00 atm NO2(8) at 25 °C, and the following equilibrium is achieved: N2O4(8) = 2 NO2(8) 20.21 After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. (a) What is the equilibrium partial pressure of N,O4? (b) Calculate the value of K, for the reaction. (c) Calculate K, for the reaction. d. 15.39 Two different proteins X and Y are dissolved in aqueous solu- tion at 37 °C. The proteins bind in a 1:1 ratio to form XY. A solution that is initially 1.00 mM in each protein is allowed to reach equilibrium. At equilibrium, 0.20 mM of free X and 0.20 mM of free Y remain, What is K. for the reaction? 15,40 A chemist at a pharmaceutical company is measuring equi- librium constants for reactions in which drug candidate molecules bind to a protein involved in cancer. The drug molecules bind the protein in a 1:1 ratio to form a drug-pro- tein complex. The protein concentration in aqueous solution at 25°C is 1.50 X 10-6 M tein sol
At equilibrium, the vessel is found to contain 0.566 g of H2. (a) Calculate the equilibrium concentrations of H2, Br, and HBr. (b) Calculate Ke. На 0.1600 mol of H20 is placed in a 2.000-L vessel. The fol- lowing equilibrium is established at 500 K: CO2(8) + H2(8) = CO(g) + H2O(g) 15.37 A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and a) Calculate the initial partial pressures of CO2, H2, and H2O. = 3.51 atm. Calculate the equilib- (b) At equilibrium RH,0 rium partial pressures of CO2, H2, and CO. (c) Calculate K. for the reaction. (d) Calculate K, for the reaction. %3D 15.38 A flask is charged with 1.500 atm of N½O4(g) and 1.00 atm NO2(8) at 25 °C, and the following equilibrium is achieved: N2O4(8) = 2 NO2(8) 20.21 After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. (a) What is the equilibrium partial pressure of N,O4? (b) Calculate the value of K, for the reaction. (c) Calculate K, for the reaction. d. 15.39 Two different proteins X and Y are dissolved in aqueous solu- tion at 37 °C. The proteins bind in a 1:1 ratio to form XY. A solution that is initially 1.00 mM in each protein is allowed to reach equilibrium. At equilibrium, 0.20 mM of free X and 0.20 mM of free Y remain, What is K. for the reaction? 15,40 A chemist at a pharmaceutical company is measuring equi- librium constants for reactions in which drug candidate molecules bind to a protein involved in cancer. The drug molecules bind the protein in a 1:1 ratio to form a drug-pro- tein complex. The protein concentration in aqueous solution at 25°C is 1.50 X 10-6 M tein sol
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...
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Question 15.38
Transcribed Image Text:At equilibrium, the vessel is found to contain 0.566 g
of H2. (a) Calculate the equilibrium concentrations of
H2, Br, and HBr. (b) Calculate Ke.
На
0.1600 mol of H20 is placed in a 2.000-L vessel. The fol-
lowing equilibrium is established at 500 K:
CO2(8) + H2(8) = CO(g) + H2O(g)
15.37 A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and
a) Calculate the initial partial pressures of CO2, H2, and H2O.
= 3.51 atm. Calculate the equilib-
(b) At equilibrium RH,0
rium partial pressures of CO2, H2, and CO. (c) Calculate K.
for the reaction. (d) Calculate K, for the reaction.
%3D
15.38 A flask is charged with 1.500 atm of N½O4(g) and 1.00 atm
NO2(8) at 25 °C, and the following equilibrium is achieved:
N2O4(8) = 2 NO2(8)
20.21
After equilibrium is reached, the partial pressure of NO2
is 0.512 atm. (a) What is the equilibrium partial pressure
of N,O4? (b) Calculate the value of K, for the reaction.
(c) Calculate K, for the reaction.
d.
15.39 Two different proteins X and Y are dissolved in aqueous solu-
tion at 37 °C. The proteins bind in a 1:1 ratio to form XY. A
solution that is initially 1.00 mM in each protein is allowed
to reach equilibrium. At equilibrium, 0.20 mM of free X and
0.20 mM of free Y remain, What is K. for the reaction?
15,40 A chemist at a pharmaceutical company is measuring equi-
librium constants for reactions in which drug candidate
molecules bind to a protein involved in cancer. The drug
molecules bind the protein in a 1:1 ratio to form a drug-pro-
tein complex. The protein concentration in aqueous solution
at 25°C is 1.50 X 10-6 M
tein sol
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