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Chhaya Baalkrishan Mammen
Asked: 2022-11-03T17:17:24+05:30 In:

The enthalpy and entropy change for the reaction
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)` are 30 kJ `mol^(-1)` and `105 JK^(-1) mol^(-1)` respectively. The temperature at which the reaction will be in equilibrium is
A. 450 K
B. 300 K
C. 285.7 K
D. 273 K

The enthalpy and entropy change for the reaction
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)` are 30 kJ `mol^(-1)` and `105 JK^(-1) mol^(-1)` respectively. The temperature at which the reaction will be in equilibrium is
A. 450 K
B. 300 K
C. 285.7 K
D. 273 K
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  1. Correct Answer – C

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Aslam Sohail Raval
Asked: 2022-11-02T07:25:49+05:30 In:

The enthalpy and entropy change for the reaction,
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)`
are `30KJmol^(-1)` and `105JK^(-1)mol^(-1)` respectively. The temperature at which the raction will be in equilibrium is:
A. 300 K
B. 285.7 K
C. 273 K
D. 450 K

The enthalpy and entropy change for the reaction,
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)`
are `30KJmol^(-1)` and `105JK^(-1)mol^(-1)` respectively. The temperature at which the raction will be in equilibrium is:
A. 300 K
B. 285.7 K
C. 273 K
D. 450 K
Parabola
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1 Answer

  1. Correct Answer – B
    `DeltaG=DeltaH-T Delta S`

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Parveen Ahluwalia
Asked: 2022-11-02T02:19:18+05:30 In:

The enthalpy and entropy change for the reaction,
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)`
are `30KJmol^(-1)` and `105JK^(-1)mol^(-1)` respectively. The temperature at which the raction will be in equilibrium is:
A. `450 K`
B. `300 K`
C. `285.7 K`
D. `273 K`

The enthalpy and entropy change for the reaction,
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)`
are `30KJmol^(-1)` and `105JK^(-1)mol^(-1)` respectively. The temperature at which the raction will be in equilibrium is:
A. `450 K`
B. `300 K`
C. `285.7 K`
D. `273 K`
Parabola
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Leave an answer

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1 Answer

  1. Correct Answer – C
    According to thermodynamics,
    `Delta G = Delta H – T Delta S`
    At equilibrium (by definition), `Delta G = 0`. Thus,
    ` 0 = Delta H – T Delta S`
    or `T = (Delta H)/(Delta S)`
    `= (30 xx 10^(3) J mol^(-1))/(105 J K^(-1) mol^(-1))`
    `285.7 K`

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