(A) For an isothermal reversible expansion of an ideal gas,the change in internal energy $\Delta U = 0$.According to the first law of thermodynamics,$

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(A) For an isothermal reversible expansion of an ideal gas,the change in internal energy $\Delta U = 0$.According to the first law of thermodynamics,$\Delta U = q + w$.Since $\Delta U = 0$,we have $q = -w$.Given that the system absorbs $208 \ J$ of heat,$q = +208 \ J$.Therefore,$w = -q = -208 \ J$.Thus,the values are $q = +208 \ J$ and $w = -208 \ J$.

Class 11 Chemistry Thermodynamics First law of thermodynamics

Medium

$A$ piston filled with $0.04 \ mol$ of an ideal gas expands reversibly from $50.0 \ mL$ to $375 \ mL$ at a constant temperature of $37.0 \ ^oC$. As it does so,it absorbs $208 \ J$ of heat. The values of $q$ and $w$ for the process will be
$(R = 8.314 \ J/mol \ K) \ (\ln 7.5 = 2.01)$

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A
$q = +208 \ J, \ w = -208 \ J$
B
$q = -208 \ J, \ w = -208 \ J$
C
$q = -208 \ J, \ w = +208 \ J$
D
$q = +208 \ J, \ w = +208 \ J$

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$A$ piston filled with $0.04 \ mol$ of an ideal gas expands reversibly from $50.0 \ mL$ to $375 \ mL$ at a constant temperature of $37.0 \ ^oC$. As it does so,it absorbs $208 \ J$ of heat. The values of $q$ and $w$ for the process will be$(R = 8.314 \ J/mol \ K) \ (\ln 7.5 = 2.01)$

Similar Questions

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

When one mole of $NH_3$ gas and one mole of $HCl$ gas are mixed in a closed container to form ammonium chloride gas,which of the following is true?

What is the value of $\Delta H - \Delta U$ for the formation of $2$ moles of ammonia from $H_{2(g)}$ and $N_{2(g)}$?

The relation between $\Delta H$ and $\Delta U$ for the reaction $2 SO_{3(g)} \longrightarrow 2 SO_{2(g)} + O_{2(g)}$ is:

$A$ system receives $224 \ J$ of heat and does $156 \ J$ of work. Calculate the change in internal energy. (in $J$)

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$A$ piston filled with $0.04 \ mol$ of an ideal gas expands reversibly from $50.0 \ mL$ to $375 \ mL$ at a constant temperature of $37.0 \ ^oC$. As it does so,it absorbs $208 \ J$ of heat. The values of $q$ and $w$ for the process will be
$(R = 8.314 \ J/mol \ K) \ (\ln 7.5 = 2.01)$