Calculate the entropy change in surroundings when 1.00 mol of \( H_2O\)(l) is formed under standard conditions. \( Δ_f H^ Θ= –286 kJ mol^{–1}.\)

Asked by Abhisek | 1 year ago |  132

1 Answer

Solution :-

It is given that \( −286\;kJmol^{−1}​​​​​​​ \)of heat is evolved on the formation of 1 mol of H2O(l) . Thus, an equal amount of heat will be absorbed by the surroundings.

Thus, the same heat will be absorbed by surrounding \( q_{surr}\) 

\( +286\;kJmol^{-1}.\)

Now, \( \Delta S_{surr} = \dfrac{q_{surr}}{7} \)

\( \dfrac{286kJmol^{-1}}{298K}\)

Therefore, \( \Delta S_{surr} = 959.73Jmol^{-1}K^{-1}\)

Answered by Pragya Singh | 1 year ago

Related Questions

Comment on the thermodynamic stability of NO(g), given,

(\( \dfrac{1}{2}\))N2(g) + (\( \dfrac{1}{2}\))O2(g) → NO(g)\( \Delta _{r}H^{\Theta } = 90kJmol^{-1}\)

NO(g) + (\( \dfrac{1}{2}\))O2(g) → NO2(g)\( \Delta _{r}H^{\Theta } = -74kJmol^{-1}\)

Class 11 Chemistry Thermodynamics View Answer

The equilibrium constant for a reaction is 10. What will be the value of ∆G0? R = 8.314 JK–1 mol–1, T = 300 K.

Class 11 Chemistry Thermodynamics View Answer

For the reaction

2A(g) + B(g)→ 2D(g)

\( \Delta U^{\Theta } = -10.5 kJ \;and \;\Delta S^{\Theta } = -44.1JK^{-1}\)

Calculate \( \Delta G^{\Theta }\) for the reaction, and predict whether the reaction may occur spontaneously.

Class 11 Chemistry Thermodynamics View Answer

For the reaction

2Cl(g)→ Cl2(g)

What are the signs of \( \Delta S\; and \;\Delta H\)?

Class 11 Chemistry Thermodynamics View Answer

For the reaction at 298K,

2A + B → C

\( \Delta H = 400 kJ mol^{-1}\)

\( \Delta H = 0.2 kJ mol^{-1}K^{-1}\)

At what temperature will the reaction become spontaneous considering \( \Delta S\; and\; \Delta H\) to be constant over the temperature range?

Class 11 Chemistry Thermodynamics View Answer