What is the equilibrium partial pressure of each gas present in the given reaction mixture?

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Marcel · Answer

Equilibrium Partial Pressures Calculation:  The given equilibrium reaction is: 1 CH4(g) + 2 H2S(g) ⇌ 1 CS2(g) + 4 H2(g)  The equilibrium partial pressures of CH4, H2S, CS2, and H2 are calculated as follows: Peq(CH4) = 0.1136 atm Peq(H2S) = 0.08024 atm Peq(CS2) = 0.1091 atm Peq(H2) = 0.0627 atm  To calculate these equilibrium partial pressures, we first determine the moles of each gas before and after equilibrium. Then, we use the given equilibrium constant (Kc) and the expression for Kc to solve for the change in concentration (x) at equilibrium. Finally, we substitute the value of x back into the equilibrium expressions for each gas to find their equilibrium partial pressures.  Now, let's look at the detailed calculation steps:  Step 1: Writing Moles Table Species   Moles Before Equilibrium   Moles at Equilibrium CH4(g)   0.1209                     0.1209 - x H2S(g)   0.09478                    0.09478 - 2x CS2(g)   0.1018                     0.1018 + x H2(g)    0.03230                    0.03230 + 4x  Where x is the change in concentration (in mol L-1) at equilibrium.  Step 2: Calculation Using Kc Expression Kc = [CS2] [H2]^4 / [CH4] [H2S]^2 Kc = {(0.1018 + x) (0.03230 + 4x)^4} / {(0.1209 - x) (0.09478 - 2x)^2}  Given Kc = 8.02 × 10-2, we solve the above equation for x.  Step 3: Equilibrium Partial Pressures Calculation At equilibrium: Peq(CH4) = 0.1209 - x = 0.1136 atm Peq(H2S) = 0.09478 - 2x = 0.08024 atm Peq(CS2) = 0.1018 + x = 0.1091 atm Peq(H2) = 0.03230 + 4x = 0.0627 atm  Therefore, the equilibrium partial pressures of CH4, H2S, CS2, and H2 are determined to be: Peq(CH4) = 0.1136 atm Peq(H2S) = 0.08024 atm Peq(CS2) = 0.1091 atm Peq(H2) = 0.0627 atm

Atmospheric Pressure Calculation Using Equilibrium Partial Pressures

Equilibrium Partial Pressures Calculation:

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