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Endothermic reactions, having DeltaS = +...

Endothermic reactions, having `DeltaS = +ve` masy be spontaneous if

A

`DeltaH gt T DeltaS`

B

`DeltaH lt T DeltaS`

C

`DeltaH = T DeltaS`

D

`T` is very high

Text Solution

AI Generated Solution

To determine the conditions under which an endothermic reaction (where ΔH > 0 and ΔS > 0) can be spontaneous, we can analyze the Gibbs free energy equation: ### Step-by-Step Solution: 1. **Understand the Gibbs Free Energy Equation**: The spontaneity of a reaction can be determined using the Gibbs free energy equation: \[ \Delta G = \Delta H - T \Delta S ...
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Knowledge Check

  • In endothermic reactions,

    A
    reactants have more energy than products
    B
    reactants have less energy than products
    C
    reactants and products have same energy
    D
    reactants have lower temperature than products.

  • Decrease in free energy of a reacting system indicates: an exothermic reaction an endothermic reaction a spontaneous reaction a slow reaction.

    A
    an exothermic reaction
    B
    an endothermic reaction
    C
    a spontaneous reaction
    D
    a slow reaction.

  • Dissolution of ammonium chloride in water is an endothermic reaction, yet it is a spontaneous process. This is due to the fact that

    A
    `DeltaH" is "+ve, DeltaS" is "-ve`
    B
    `DeltaH" is "-ve, DeltaS" is "+ve`
    C
    `DeltaH" is "+ve, DeltaS" is "+ve and DeltaH lt TDeltaS`
    D
    `DeltaH" is "+ve and DeltaH gt T DeltaS`

    • Similar Questions

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    In an endothermic reaction, the value of DeltaH is

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    Assertion (A): May endothermic reactions that are not spontaneous at room temperature become spontaneous at high temperature. Reason (R ) : Entropy of the system increases with increase in temperature.

    For an endothermic reaction, where Delta H represents the enthalpy of reaction in kJ mol^(-1) , the minimum value for the energy of activation will be

    Comment on the following statements. Endothermic reactions have higher activation energies than exothermic reactions.

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