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प्रश्न
The equilibrium constant for a reaction is 10. What will be the value of ΔG⊝? R = 8.314 JK–1 mol–1,T = 300 K.
उत्तर
From the expression,
ΔG⊝ = –2.303 RT logKeq
ΔG⊝ for the reaction,
= (2.303) (8.314 JK–1 mol–1) (300 K) log10
= - 5744.14 Jmol–1
= - 5.744 kJ mol–1
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संबंधित प्रश्न
At 298 K. Kp for the reaction \[\ce{N2 O4 (g) ⇌ 2NO2 (g)}\] is 0.98. Predict whether the reaction is spontaneous or not.
Which quantity out of ∆rG and ∆rGΘ will be zero at equilibrium?
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| ∆ (Parameters) \[\ce{∆_rH^Θ, ∆_rS^Θ, ∆_rG^Θ}\] |
Description |
| (i) \[\ce{+ – +}\] | (a) Non-spontaneous at high temperature |
| (ii) \[\ce{– – + at high T}\] | (b) Spontaneous at all temperatures |
| (iii) \[\ce{– + –}\] | (c) Non-spontaneous at all temperatures |
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