Open Question
For the reaction 2 A(g) ⇌ B(g) + 2 C(g), a reaction vessel initially contains only A at a pressure of PA = 255 mmHg. At equilibrium, PA = 55 mmHg. Calculate the value of Kp. (Assume no changes in volume or temperature.)
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 45
Consider the reaction: H2(g) + I2(g) ⇌ 2 HI(g). A reaction mixture in a 3.67-L flask at a certain temperature initially contains 0.763 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.4 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature.
Verified step by step guidance1
Convert the initial masses of H2 and I2 to moles using their molar masses: \( \text{moles of } H_2 = \frac{0.763 \text{ g}}{2.02 \text{ g/mol}} \) and \( \text{moles of } I_2 = \frac{96.9 \text{ g}}{253.8 \text{ g/mol}} \).
Convert the mass of HI at equilibrium to moles using its molar mass: \( \text{moles of } HI = \frac{90.4 \text{ g}}{127.9 \text{ g/mol}} \).
Determine the change in moles of HI from the initial state to equilibrium, and use stoichiometry to find the changes in moles of H2 and I2.
Calculate the equilibrium moles of H2 and I2 by subtracting the change in moles from their initial moles.
Use the equilibrium concentrations (moles/volume) of H2, I2, and HI to calculate the equilibrium constant \( K_c = \frac{[HI]^2}{[H_2][I_2]} \).
Related Practice
Open Question
Consider the reaction: Fe3+ (aq) + SCN- (aq) ⇌ FeSCN2+ (aq). A solution is made containing an initial [Fe3+] of 1.0*10^-3 M and an initial [SCN-] of 8.0*10^-4 M. At equilibrium, [FeSCN2+] = 1.7*10^-4 M. Calculate the value of the equilibrium constant (Kc).
Open Question
Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g). A reaction mixture is made containing an initial [SO2Cl2] of 0.020 M. At equilibrium, [Cl2] = 1.2*10^-2 M. Calculate the value of the equilibrium constant (Kc).
Open Question
Consider the reaction: CO(g) + 2 H2(g) ⇌ CH3OH(g). A reaction mixture in a 5.19-L flask at a certain temperature contains 26.9 g CO and 2.34 g H2. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature.
Textbook Question
Consider the reaction: NH4HS(s) ⇌ NH3(g) + H2S(g) At a certain temperature, Kc = 8.5⨉10-3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached?
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Open Question
Consider the reaction: 2H2S(g) ⇌ 2H2(g) + S2(g). Kp = 2.4 * 10^-4 at 1073K. A reaction mixture contains 0.112 atm of H2, 0.055 atm of S2, and 0.445 atm of H2S. Is the reaction mixture at equilibrium? If not, in what direction will the reaction proceed?