For the reaction N_{2(g)} + 3H_{2(g)} to 2NH_ | vedclass

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

Question

(A) 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

$\Delta H = \Delta U - 2RT$

Vedclass · Answer

(A) 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 the reaction $N_{2(g)} + 3H_{2(g)} 	o 2NH_{3(g)}$,the number of moles of gaseous products is $n_p = 2$ and the number of moles of gaseous reactants is $n_r = 1 + 3 = 4$. Therefore,the change in the number of gaseous moles is $\Delta n_g = n_p - n_r = 2 - 4 = -2$. Substituting this value into the equation: $\Delta H = \Delta U + (-2)RT = \Delta U - 2RT$.

For the reaction $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$,the relationship between $\Delta H$ and $\Delta U$ is:

Similar Questions

An ideal gas undergoes a cyclic transformation starting from the point $A$ and coming back to the same point by tracing the path $A$ $\rightarrow B$ $\rightarrow C$ $\rightarrow D$ $\rightarrow A$ as shown in the three cases above. Choose the correct option regarding $\Delta U$.

What is molar enthalpy of vaporization?

Any series of operations so carried out that at the end,the system is back to its initial state is called:

Which of the following is true for an adiabatic process?

$1 \text{ mole}$ of an ideal gas is compressed isothermally and reversibly from an initial pressure $x \text{ kPa}$ to a final pressure $2x \text{ kPa}$ at $300 \text{ K}$. Find the work done $(R = 8.314 \text{ J K}^{-1} \text{mol}^{-1})$. (in $\text{ J}$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module