For which of the following reactions,Delta H | vedclass

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

Question

(B) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U   \De

Vedclass · Accepted Answer

$2HI_{(g)} 	o H_{2(g)} + I_{2(g)}$

Vedclass · Answer

(B) The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by the equation: $\Delta H = \Delta U   \Delta n_g RT$.For $\Delta H$ to be equal to $\Delta U$,the term $\Delta n_g$ must be $0$.$\Delta n_g$ is the difference between the sum of stoichiometric coefficients of gaseous products and gaseous reactants.For option $B$: $2HI_{(g)} 	o H_{2(g)}   I_{2(g)}$,$\Delta n_g = (1   1) - 2 = 0$.Since $\Delta n_g = 0$,$\Delta H = \Delta U   0$,which means $\Delta H = \Delta U$.

For which of the following reactions,$\Delta H$ is equal to $\Delta U$ ?

Similar Questions

The relation between change in internal energy $(\Delta E)$,change in enthalpy $(\Delta H)$,and work done $(W)$ is represented as:

In an isothermal and reversible process,$1.6 \times 10^{-2} \ kg$ of $O_2$ expands from $10 \ dm^3$ to $100 \ dm^3$ at $300 \ K$. The work done in the process is: $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$ (in $J$)

The enthalpy of fusion of ice per mole is approximately $...$ $kJ / mol$.

Two moles of an ideal gas is expanded isothermally and reversibly at $300 \ K$ from $1 \ L$ to $10 \ L$. The enthalpy change in $kJ$ is

Two moles of an ideal gas is expanded isothermally from a volume of $300 \ cm^3$ to $2.5 \ dm^3$ at $298 \ K$ against a constant pressure of $1.9 \ bar$. Calculate the work done in joules. (in $J$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module