Question 7 (1 point) Consider the following reaction: $C_{(s)} + 2 H_{2(g)} \rightleftharpoons CH_{4(g)}$ The equilibrium expression is $Kc = [CH_4]/[2H_2]^2$ $Kc = [CH_4]/[H_2]^2$ $Kc = [H_2]^2 / [CH_4]$ $Kc = [CH_4] / [H_2]^2[C]$
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Given the following reaction, write the equilibrium expression: C (s) + 2 H2 (g) ↔ CH4 (g) [CH4]/[C] [H2]2 [C][H2] [CH4]/[H2]2 [H2]2[C]/[CH4]
Sri K.
At $2000 \mathrm{K}, K_{c}=0.154$ for the reaction $2 \mathrm{CH}_{4}(\mathrm{g}) \rightleftharpoons$ $\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{g}) .$ If a 1.00 L equilibrium mixture at $2000 \mathrm{K}$ contains $0.10 \mathrm{mol}$ each of $\mathrm{CH}_{4}(\mathrm{g})$ and $\mathrm{H}_{2}(\mathrm{g})$ (a) What is the mole fraction of $\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g})$ present? (b) Is the conversion of $\mathrm{CH}_{4}(\mathrm{g})$ to $\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g})$ favored at high or low pressures? (c) If the equilibrium mixture at $2000 \mathrm{K}$ is transferred from a 1.00 L flask to a 2.00 L flask, will the number of moles of $\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{g})$ increase, decrease, or remain unchanged?
Consider the following reaction for which Kc = 3.24 × 104. CH4(g) + 2 H2S(g) ⇌ CS2(g) + 4 H2(g) The initial concentrations are: [CH4] = 0.035 M, [H2S] = 0.042 M, [CS2] = 0.94 M, and [H2] = 0.16 M Select the true statement. Qc = 0.11 The reaction shifts to produce more products. Qc > Kc Qc = 100 The reaction shifts to produce more reactants.
Tianyu L.
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