Assertion (A): Formation of H_2O_{(ell)} from | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The reaction for the formation of water is: $H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(state)}$.When $H_2O$ is formed as a liquid,the ent

Vedclass · Accepted Answer

Both assertion and Reason are correct and Reason is the correct explanation of Assertion.

Vedclass · Answer

(A) The reaction for the formation of water is: $H_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow H_2O_{(state)}$.When $H_2O$ is formed as a liquid,the enthalpy of condensation (releasing energy) is added to the enthalpy of formation of gaseous water.Since the formation of $H_2O_{(\ell)}$ involves the release of energy during the phase change from gas to liquid,the overall process is more exothermic.Thus,the Assertion is correct.The Reason states that $H_2O_{(\ell)}$ has stronger intermolecular forces (hydrogen bonding) compared to $H_2O_{(g)}$,making it more stable.This increased stability due to intermolecular attraction is the fundamental reason why the formation of the liquid state releases more energy.Therefore,both Assertion and Reason are correct,and the Reason is the correct explanation of the Assertion.

Assertion $(A)$: Formation of $H_2O_{(\ell)}$ from $H_{2(g)}$ and $O_{2(g)}$ is more exothermic than formation of $H_2O_{(g)}$ from $H_{2(g)}$ and $O_{2(g)}$.
Reason $(R)$: $H_2O_{(\ell)}$ has more attraction force than $H_2O_{(g)}$ and it is more stable than $H_2O_{(g)}$.

Similar Questions

For the reaction $H_{2(g)} + I_{2(g)} \rightarrow 2HI_{(g)}; \Delta H = 12.40 \, Kcal$,the heat of formation of $HI$ is ....... $Kcal$.

Find the value of enthalpy of formation of $PCl_5(s)$ given the following thermochemical equations:
$1) \frac{1}{2} P_{4(s)} + 3Cl_{2(g)} \to 2PCl_3(\ell) ; \Delta H = -635 \ kJ$
$2) PCl_3(\ell) + Cl_{2(g)} \to PCl_{5(s)} ; \Delta H = -137 \ kJ$

The enthalpy change for the reaction,$H_{2(g)} + C_2H_{4(g)} \to C_2H_{6(g)}$ is $......$ $kcal \ mol^{-1}$. The bond energies are,$[e_{H-H} = 103, e_{C-H} = 99, e_{C-C} = 80]$ and $[e_{C=C} = 145] \ kcal \ mol^{-1}$.

If the bond energies of $H-H$,$Br-Br$ and $H-Br$ are $433$,$192$ and $364 \ kJ \ mol^{-1}$ respectively,then $\Delta H^{\circ}$ for the reaction: $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$ is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Assertion $(A)$: Formation of $H_2O_{(\ell)}$ from $H_{2(g)}$ and $O_{2(g)}$ is more exothermic than formation of $H_2O_{(g)}$ from $H_{2(g)}$ and $O_{2(g)}$.Reason $(R)$: $H_2O_{(\ell)}$ has more attraction force than $H_2O_{(g)}$ and it is more stable than $H_2O_{(g)}$.