(A) Heat absorbed by the steel boiler: $q_1 = m_1 s_1 \Delta T = 900 \times 0.11 \times (100 - 10) = 900 \times 0.11 \times 90 = 8910 \, kcal$. Heat a

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(A) Heat absorbed by the steel boiler: $q_1 = m_1 s_1 \Delta T = 900 \times 0.11 \times (100 - 10) = 900 \times 0.11 \times 90 = 8910 \, kcal$. Heat absorbed by the water: $q_2 = m_2 s_2 \Delta T = 400 \times 1.0 \times (100 - 10) = 400 \times 1.0 \times 90 = 36000 \, kcal$. Total net heat required $(Q_{net})$ = $q_1 + q_2 = 8910 + 36000 = 44910 \, kcal$. Since only $70 \%$ of the supplied heat is utilized,let $Q_{total}$ be the total heat supplied: $0.70 \times Q_{total} = 44910 \, kcal$. $Q_{total} = \frac{44910}{0.70} = 64157.14 \, kcal \approx 64157 \, kcal$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Difficult

$A$ steel steam boiler has a mass of $900 \, kg$ and contains $400 \, kg$ of water. If the boiler and water receive only $70 \%$ of the heat supplied,how much heat in $kcal$ is required to raise the temperature of the boiler and water from $10 \, ^oC$ to $100 \, ^oC$? (Specific heat of steel = $0.11 \, kcal/kg \cdot K$,Specific heat of water = $1.0 \, kcal/kg \cdot K$)

A
$64157$
B
$64.157$
C
$5675$
D
$3842$

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Mix Examples-Thermodynamics and Thermochemistry

The enthalpy of vaporization of a liquid at $500 \, K$ and $1 \, atm$ pressure is $10 \, kcal \, mol^{-1}$. The change in internal energy $(\Delta U)$ for $3 \, moles$ of the liquid at the same temperature and pressure is ............ $kcal$.

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In an adiabatic process,the work involved during expansion or compression of an ideal gas is given by

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The difference between $\Delta H$ and $\Delta U$ $(\Delta H - \Delta U),$ when the combustion of one mole of heptane $(l)$ is carried out at a temperature $T$ is equal to (in $,RT$)

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At $25$ $^\circ C$ and $1$ $atm$ pressure,the enthalpies of formation of $C_2H_4(g)$,$CO_2(g)$,and $H_2O(l)$ are $52$,$-394$,and $-286 \, kJ \, mol^{-1}$ respectively. The enthalpy of combustion of $C_2H_4$ is ....... $kJ \, mol^{-1}$.

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Consider the following statements:
Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is:

MediumAP EAMCET 2025

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The enthalpy of vaporization of a liquid at $500 \, K$ and $1 \, atm$ pressure is $10 \, kcal \, mol^{-1}$. The change in internal energy $(\Delta U)$ for $3 \, moles$ of the liquid at the same temperature and pressure is ............ $kcal$.

In an adiabatic process,the work involved during expansion or compression of an ideal gas is given by

The difference between $\Delta H$ and $\Delta U$ $(\Delta H - \Delta U),$ when the combustion of one mole of heptane $(l)$ is carried out at a temperature $T$ is equal to (in $,RT$)

At $25$ $^\circ C$ and $1$ $atm$ pressure,the enthalpies of formation of $C_2H_4(g)$,$CO_2(g)$,and $H_2O(l)$ are $52$,$-394$,and $-286 \, kJ \, mol^{-1}$ respectively. The enthalpy of combustion of $C_2H_4$ is ....... $kJ \, mol^{-1}$.

Consider the following statements:Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.The correct answer is:

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Consider the following statements:
Statement-$I$: Both internal energy $(U)$ and work $(w)$ are state functions.
Statement-$II$: During the free expansion of an ideal gas into vacuum,the work done is zero.
The correct answer is: