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प्रश्न
Match the following parameters with description for spontaneity
| ∆ (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 |
उत्तर
| ∆ (Parameters) \[\ce{∆_rH^Θ, ∆_rS^Θ, ∆_rG^Θ}\] |
Description |
| (i) \[\ce{+ – +}\] | (c) Non-spontaneous at all temperatures |
| (ii) \[\ce{– – + at high T}\] | (a) Non-spontaneous at high temperature |
| (iii) \[\ce{– + –}\] | (b) Spontaneous at all temperatures |
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संबंधित 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.
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?
Assertion (A): Spontaneous process is an irreversible process and may be reversed by some external agency.
Reason (R): Decrease in enthalpy is a contributory factor for spontaneity.
\[\ce{∆G}\] is net energy available to do useful work and is thus a measure of “free energy”. Show mathematically that ∆G is a measure of free energy. Find the unit of \[\ce{∆G}\]. If a reaction has positive enthalpy change and positive entropy change, under what condition will the reaction be spontaneous?
The correct relationship between free energy change in a reaction and the corresponding equilibrium constant Kc is:
For the reaction \[\ce{A(g) -> B(g)}\], the value of equilibrium constant at 300 K and 1 atm is equal to 100.0. The value of ΔrG for the reaction at 300 K and 1 atm in J mol−1 is −xR, where x is ______. (Rounded-off to the nearest integer)
[R = 8.31 J mol−1 K−1 and ln 10 = 2.3]
The standard reaction Gibbs energy for a chemical reaction at an absolute temperature T is given by ΔG0 = A − BT where A and Bare non-zero constants. Which of the following is true about this reaction?
