The total entropy change, ΔStotal, of a reaction at 298 K is −85.0 J K−1 mol−1.
What is the value of the equilibrium constant for this reaction at 298 K?
[R = 8.31 J mol−1 K−1]
3.61 × 10−5
9.07 × 10−1
9.66 × 10−1
2.77 × 104
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The total entropy change, ΔStotal, of a reaction at 298 K is −85.0 J K−1 mol−1.
What is the value of the equilibrium constant for this reaction at 298 K?
[R = 8.31 J mol−1 K−1]
3.61 × 10−5
9.07 × 10−1
9.66 × 10−1
2.77 × 104
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The reaction shown is at equilibrium. The forward reaction is endothermic.
C (s) + CO2 (g) ⇌ 2CO (g)
the mole fraction of carbon dioxide
the partial pressure of carbon monoxide
the rate of the backward reaction
the value of Kp for the forward reaction
0.237
0.263
0.474
0.526
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The equation for the precipitation of lead(II) chloride is shown.
Pb2+ (aq) + 2Cl– (aq) ⇌ PbCl2 (s)
What are the units of the equilibrium constant, Kc?
dm9 mol–3
dm6 mol–2
mol2 dm–6
mol3 dm–9
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The water gas reaction is used in the manufacture of hydrogen.
C (s) + H2O (g) ⇌ CO (g) + H2 (g) ∆= +131.2 kJ mol−1
Kc = [CO][H2]
Kc =
Kc =
Kc =
Kc of forward reaction | Kc of reverse reaction | |||
☐ | A | increases | increases | |
☐ | B | increases | decreases | |
☐ | C | decreases | increases | |
☐ | D | decreases | decreases |
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