An ideal gas expands by performing 200 J of | vedclass

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

Question

(D) The relationship between enthalpy change $(\Delta H)$,internal energy change $(\Delta U)$,and work done $(W)$ is given by: $\Delta H = \Delta U +

Vedclass · Accepted Answer

$632$

Vedclass · Answer

(D) The relationship between enthalpy change $(\Delta H)$,internal energy change $(\Delta U)$,and work done $(W)$ is given by: $\Delta H = \Delta U + P \Delta V$. Since work done by the system during expansion is $W = -P \Delta V$,we have $P \Delta V = -W$. Therefore,$\Delta H = \Delta U - W$. Given: Internal energy change $\Delta U = +432 \ J$. Work done by the gas $W = 200 \ J$. Since the gas performs work,the work done on the system is $-200 \ J$. Substituting the values: $\Delta H = 432 \ J - (-200 \ J) = 432 \ J + 200 \ J = 632 \ J$.

An ideal gas expands by performing $200 \ J$ of work,during this internal energy increases by $432 \ J$. What is the enthalpy change (in $J$)?

Similar Questions

Which of the following statements regarding the first law of thermodynamics is correct?

If $\Delta H$ is the change in enthalpy and $\Delta E$ is the change in internal energy accompanying a gaseous reaction,which of the following is true?

If the heat of combustion of isobutane at constant volume is $Q_v$,what will be the heat of combustion of one mole of isobutane at constant pressure and standard conditions? (Given: $\Delta n_g = -3.5$)

What is the internal energy change when $62 \ J$ of work is done on the system and $128 \ J$ of heat is transferred to the surrounding (in $J$)?

The $\Delta U^o$ of combustion of $CH_{4(g)}$ at a certain temperature is $-393 \ kJ/mol$. Then the value of $\Delta H^o$ is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module