If one mole of ammonia and one mole of hydrog | vedclass

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

Question

(C) The chemical reaction is: $NH_3(g) + HCl(g) \rightarrow NH_4Cl(g)$The relationship between enthalpy change $(\Delta H)$ and internal energy change

Vedclass · Accepted Answer

$\Delta H < \Delta U$

Vedclass · Answer

(C) The chemical reaction is: $NH_3(g) + HCl(g) ightarrow NH_4Cl(g)$The relationship between enthalpy change $(\Delta H)$ and internal energy change $(\Delta U)$ is given by: $\Delta H = \Delta U + \Delta n_g RT$Where $\Delta n_g$ is the change in the number of moles of gaseous species.$\Delta n_g = (	ext{moles of gaseous products}) - (	ext{moles of gaseous reactants})$$\Delta n_g = 1 - (1 + 1) = 1 - 2 = -1$Substituting this into the equation: $\Delta H = \Delta U - RT$Since $RT$ is positive,it follows that $\Delta H < \Delta U$.

If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas,then

Similar Questions

If a gas expands adiabatically from $1 \, L$ to $12 \, L$ against a constant external pressure of $0.75 \, atm$,the $\Delta U$ of the gas is .... $J$. (in $.9$)

When $100 \ cal$ of heat is supplied to a system,the work done by the system is $300 \ J$. The change in internal energy of the system is ..... $J$.

The relation $q = -w$ is $NOT$ true for which of the following processes?

At constant $T$ and $P$,which one of the following statements is correct for the reaction,$CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$?

At $1 \ bar$ pressure,a gas has a volume of $0.6 \ L$. If this gas gains $122 \ J$ of heat at $1 \ bar$ pressure,its volume becomes $2 \ L$. Calculate its internal energy change. [Given: $1 \ L \cdot bar = 101.32 \ J$]

Vedclass Test Series

Exam Paper Generator

Online Exam Module