The enthalpies of formation of gaseous N_2O a | vedclass

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

Question

(B) The enthalpy change of the reaction is calculated using the formula: $\Delta H_{r}^{\circ} = \sum \Delta H_{f}^{\circ}(	ext{products}) - \sum \De

Vedclass · Accepted Answer

$+98 \ kJ$

Vedclass · Answer

(B) The enthalpy change of the reaction is calculated using the formula: $\Delta H_{r}^{\circ} = \sum \Delta H_{f}^{\circ}(	ext{products}) - \sum \Delta H_{f}^{\circ}(	ext{reactants})$.For the reaction $N_2O_{(g)} + \frac{1}{2} O_{2(g)} ightarrow 2 NO_{(g)}$,the expression is: $\Delta H_{r}^{\circ} = [2 	imes \Delta H_{f}^{\circ}(NO)] - [\Delta H_{f}^{\circ}(N_2O) + \frac{1}{2} 	imes \Delta H_{f}^{\circ}(O_2)]$.Given that $\Delta H_{f}^{\circ}(O_2) = 0 \ kJ \ mol^{-1}$ (standard state of an element),$\Delta H_{f}^{\circ}(N_2O) = 82.0 \ kJ \ mol^{-1}$,and $\Delta H_{f}^{\circ}(NO) = 90.0 \ kJ \ mol^{-1}$.Substituting the values: $\Delta H_{r}^{\circ} = [2 	imes 90.0] - [82.0 + 0] = 180.0 - 82.0 = +98.0 \ kJ$.

The enthalpies of formation of gaseous $N_2O$ and $NO$ at $298 \ K$ are $82.0$ and $90.0 \ kJ \ mol^{-1}$ respectively. The enthalpy change of the reaction $N_2O_{(g)} + \frac{1}{2} O_{2(g)} \rightarrow 2 NO_{(g)}$ is

Similar Questions

$10 \ g$ each of $NH_3, N_2, Cl_2$ and $H_2S$ are expanded isothermally and reversibly at the same temperature. Identify the gas that performs maximum work.

The standard entropies of $X_2, Y_2$ and $XY_3$ are $60, 40$ and $50 \ J \ K^{-1} \ mol^{-1}$ respectively. For the reaction $X_2 + 3Y_2 \rightleftharpoons 2XY_3; \Delta H = -60 \ kJ$ to be at equilibrium,the temperature should be.....$K$

The heat change for the following reaction at $298 \ K$ and at constant pressure is $+ 7.3 \ kcal$. $A_2B_{(s)} \to 2A_{(s)} + 1/2 \ B_{2(g)}$,$\Delta H = + 7.3 \ kcal$. The heat change at constant volume would be

For the reaction $X_2Y_{4(l)} \rightarrow 2XY_{2(g)}$ at $300 \ K$,the values of $\Delta U$ and $\Delta S$ are $2 \ kcal$ and $20 \ cal \ K^{-1}$ respectively. The value of $\Delta G$ for the reaction is (in $cal$)

Which of the following relations between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is correct for the given reactions?

Vedclass Test Series

Exam Paper Generator

Online Exam Module