At 298 K,what is the value of Delta H - Delt | vedclass

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

Question

(B) The chemical reaction is: $C_{(s)} + \frac{1}{2} O_{2(g)} \rightarrow CO_{(g)}$The change in the number of moles of gaseous species is $\Delta n_g

Vedclass · Accepted Answer

$1238.78$

Vedclass · Answer

(B) The chemical reaction is: $C_{(s)} + \frac{1}{2} O_{2(g)} ightarrow CO_{(g)}$The change in the number of moles of gaseous species is $\Delta n_g = n_{p(g)} - n_{r(g)} = 1 - 0.5 = 0.5 \ mol$.From the first law of thermodynamics,the relationship between enthalpy change and internal energy change is $\Delta H = \Delta E + \Delta n_g RT$.Therefore,$\Delta H - \Delta E = \Delta n_g RT$.Substituting the values: $\Delta H - \Delta E = 0.5 	imes 8.314 	imes 298 = 1238.78 \ J \ mol^{-1}$.

At $298 \ K$,what is the value of $\Delta H - \Delta E$ in $J \ mol^{-1}$ when $1 \ mol$ of carbon monoxide gas is formed from its elements in their standard states? $[R = 8.314 \ J \ K^{-1} \ mol^{-1}]$

Similar Questions

One mole of an ideal gas is allowed to expand reversibly and adiabatically from a temperature of $27\,^{\circ}C$. If the work done during the process is $3\, kJ$,then the final temperature of the gas is $...\, K$.

$A$ gas is allowed to expand in an insulated container against a constant external pressure of $2.5 \ atm$ from $2.5 \ L$ to $4.5 \ L$. The change in internal energy of the gas in joules is: (in $J$)

For the reaction $CO_{(g)} + \frac{1}{2} O_{2(g)} \to CO_{2(g)}$,which of the following is true?

When a gas undergoes adiabatic expansion,it cools down because:

When $1 \ mole$ of gas is heated at constant volume and heat supplied is $500 \ J$,then which of the following is correct?

Vedclass Test Series

Exam Paper Generator

Online Exam Module