2) Consider the reaction for the decomposition of hydrogen disulfide: 2 H2S (g) ⇌2 H2 (g) + S2 (g) KP=2.4x10-4 at 1073 K A reaction vessel initially contains 0.752 atm of H2S at 1073 K. Find the equilibrium concentrations of H2 and S2. 3) The reaction in question 2 is then carried out at the same temperature but the initial pressures were 0.20 atm for H2 and 0.40 atm for S2. Calculate the equilibrium concentrations.
2) Consider the reaction for the decomposition of hydrogen disulfide: 2 H2S (g) ⇌2 H2 (g) + S2 (g) KP=2.4x10-4 at 1073 K A reaction vessel initially contains 0.752 atm of H2S at 1073 K. Find the equilibrium concentrations of H2 and S2. 3) The reaction in question 2 is then carried out at the same temperature but the initial pressures were 0.20 atm for H2 and 0.40 atm for S2. Calculate the equilibrium concentrations.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2) Consider the reaction for the decomposition of hydrogen disulfide:
2 H2S (g) ⇌2 H2 (g) + S2 (g) KP=2.4x10-4 at 1073 K
A reaction vessel initially contains 0.752 atm of H2S at 1073 K. Find the equilibrium concentrations of H2 and S2.
3) The reaction in question 2 is then carried out at the same temperature but the initial pressures were
0.20 atm for H2 and 0.40 atm for S2. Calculate the equilibrium concentrations.
Expert Solution
Step 1
To find the equilibrium concentrations of H2 and S2, we can use the equation of reaction quotient (Q). The equation of Q is given by:
where P represents the pressure of each gas in the atmosphere.
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