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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Ch.15 - Chemical Equilibrium
Chapter 15, Problem 6
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.
Verified step by step guidance1
Convert the initial partial pressures from torr to atm by dividing each by 760, since 1 atm = 760 torr.
Set up an ICE (Initial, Change, Equilibrium) table to track the changes in partial pressures of each species. Let the change in pressure for CO and H2O be \(-x\), and for CO2 and H2 be \(+x\).
Write the expression for the equilibrium constant \(K_p\) in terms of partial pressures: \(K_p = \frac{P_{CO_2} \cdot P_{H_2}}{P_{CO} \cdot P_{H_2O}}\).
Substitute the equilibrium expressions from the ICE table into the \(K_p\) expression and solve for \(x\).
Calculate the equilibrium partial pressures by substituting \(x\) back into the expressions for each species: \(P_{CO} = P_{CO, initial} - x\), \(P_{H_2O} = P_{H_2O, initial} - x\), \(P_{CO_2} = x\), and \(P_{H_2} = x\).
Related Practice
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
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?
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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Textbook Question
Find and fix each mistake in the equilibrium constant expressions. a. 2 H2S(g) ⇌ 2 H2(g) + S2(g) K = [H2][S2]/[H2S]
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