Find the enthalpy of formation of the OH^- io | vedclass

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

Question

(B) The enthalpy of formation of $H_2O_{(l)}$ is given as $\Delta H_f(H_2O, l) = -286.20 \ KJ/mol$.For the reaction: $H_2O_{(l)} 	o H^+_{(aq)} + OH^-

Vedclass · Accepted Answer

$-228.88$

Vedclass · Answer

(B) The enthalpy of formation of $H_2O_{(l)}$ is given as $\Delta H_f(H_2O, l) = -286.20 \ KJ/mol$.For the reaction: $H_2O_{(l)} 	o H^+_{(aq)} + OH^-_{(aq)}$,the enthalpy change is $\Delta H_r = 57.32 \ KJ/mol$.The enthalpy of reaction is calculated as:$\Delta H_r = [\Delta H_f(H^+, aq) + \Delta H_f(OH^-, aq)] - \Delta H_f(H_2O, l)$By convention,the enthalpy of formation of $H^+_{(aq)}$ is $0 \ KJ/mol$.Substituting the values:$57.32 = [0 + \Delta H_f(OH^-, aq)] - (-286.20)$$57.32 = \Delta H_f(OH^-, aq) + 286.20$$\Delta H_f(OH^-, aq) = 57.32 - 286.20 = -228.88 \ KJ/mol$.

Find the enthalpy of formation of the $OH^-$ ion in $KJ$ at $25^\circ C$ from the following data:
$H_2O_{(l)} \to H^+_{(aq)} + OH^-_{(aq)} ; \Delta H = 57.32 \ KJ$
$H_{2(g)} + \frac{1}{2} O_{2(g)} \to H_2O_{(l)} ; \Delta H = -286.20 \ KJ$

Similar Questions

The enthalpies of dissolution of $BaCl_2(s)$ and $BaCl_2 \cdot 2H_2O(s)$ are $-20.6 \ kJ \ mol^{-1}$ and $8.8 \ kJ \ mol^{-1}$ respectively. Calculate the enthalpy of hydration for the given reaction: $BaCl_2(s) + 2H_2O(l) \to BaCl_2 \cdot 2H_2O(s)$

The heat of combustion of carbon is $-393.5 \ kJ / mol$. The heat released upon the formation of $35.2 \ g$ of $CO_{2}$ from carbon and oxygen gas is

At $298 \ K$,the enthalpy of fusion of a solid $(X)$ is $2.8 \ kJ \ mol^{-1}$ and the enthalpy of vaporisation of the liquid $(X)$ is $98.2 \ kJ \ mol^{-1}$. The enthalpy of sublimation of the substance $(X)$ in $kJ \ mol^{-1}$ is $.....$ (in nearest integer).

The $\Delta H_f^o$ values for $ICl_{(g)}$,$Cl_{(g)}$,and $I_{(g)}$ are $17.57$,$121.34$,and $106.96 \, J \, mol^{-1}$ respectively. What is the bond dissociation energy of the $I-Cl$ bond in $J \, mol^{-1}$?

The atomization enthalpies of $NH_{3(g)}$ and $N_2H_{4(g)}$ are $+150 \ kJ \ mol^{-1}$ and $+310 \ kJ \ mol^{-1}$ respectively. The $\Delta H(N-N)$ bond enthalpy in $kJ \ mol^{-1}$ is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Find the enthalpy of formation of the $OH^-$ ion in $KJ$ at $25^\circ C$ from the following data:$H_2O_{(l)} \to H^+_{(aq)} + OH^-_{(aq)} ; \Delta H = 57.32 \ KJ$$H_{2(g)} + \frac{1}{2} O_{2(g)} \to H_2O_{(l)} ; \Delta H = -286.20 \ KJ$