Textbook Question
Calculate Kc for each reaction.
b. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) Kp = 7.7x1024 (at 298 K)
c. I2(g) + Cl2(g) ⇌ 2 ICl(g) Kp = 81.9 (at 298 K)
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Ch.15 - Chemical Equilibrium
Chapter 15, Problem 5
Nitrogen dioxide dimerizes according to the reaction: 2 NO2(g) ⇌ N2O4(g) Kp = 6.7 at 298 K. A 2.25-L container contains 0.055 mol of NO2 and 0.082 mol of N2O4 at 298 K. Is the reaction at equilibrium? If not, in which direction will the reaction proceed?
Verified step by step guidance1
Calculate the initial partial pressures of NO2 and N2O4 using the ideal gas law: P = (nRT)/V, where n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), T is the temperature in Kelvin, and V is the volume of the container.
Determine the reaction quotient, Qp, using the expression Qp = (P_{N2O4}) / (P_{NO2})^2, where P_{N2O4} and P_{NO2} are the partial pressures of N2O4 and NO2, respectively.
Compare the calculated Qp to the given equilibrium constant Kp. If Qp < Kp, the reaction will proceed in the forward direction to reach equilibrium. If Qp > Kp, the reaction will proceed in the reverse direction. If Qp = Kp, the reaction is at equilibrium.
Analyze the direction of the reaction based on the comparison of Qp and Kp to determine if the reaction will shift towards the formation of more products (N2O4) or reactants (NO2).
Conclude whether the reaction is at equilibrium or predict the direction in which the reaction will proceed to reach equilibrium.
Related Practice
Textbook Question
Calculate Kp for each reaction.
b. N2(g) + 3 H2(g) ⇌ 2 NH3(g) Kc = 3.7⨉108 (at 298 K)
c. N2(g) + O2(g) ⇌ 2 NO(g) Kc = 4.10⨉10-31 (at 298 K)
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Textbook Question
Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction: C(s) + 2 H2(g) ⇌ CH4(g) Which disturbance will favor CH4 at equilibrium?
a. adding more C to the reaction mixture b. adding more H2 to the reaction mixture d. lowering the volume of the reaction mixture f. adding neon gas to the reaction mixture
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Open Question
Consider the reaction: CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Kp = 0.0611 at 2000 K. A reaction mixture initially contains a CO partial pressure of 1344 torr and a H2O partial pressure of 1766 torr at 2000 K. Calculate the equilibrium partial pressures of each of the products.
Open Question
This reaction is exothermic. C6H12O6(s) + 6 O2(g) ⇌ 6 CO2(g) + 6 H2O(g). Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature?
Textbook Question
Write an expression for the equilibrium constant of each chemical equation.
a. SbCl5(g) ⇌ SbCl3(g) + Cl2(g)
b.2 BrNO(g) ⇌ 2 NO(g) + Br2(g)
c. CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g)
d. 2 CO(g) + O2(g) ⇌ 2 CO2(g)
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