(D) The total heat required $(q)$ is the sum of the heat required to raise the temperature of the liquid $(q_1)$ and the heat required for phase chang

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(D) The total heat required $(q)$ is the sum of the heat required to raise the temperature of the liquid $(q_1)$ and the heat required for phase change $(q_2)$.$q_1 = m \times c \times \Delta T$$q_1 = 1000 \, g \times 2.44 \, J \, g^{-1} \, K^{-1} \times (351.45 \, K - 293.45 \, K)$$q_1 = 1000 \times 2.44 \times 58 = 141520 \, J = 1.4152 \times 10^5 \, J$$q_2 = m \times L_v$$q_2 = 1000 \, g \times 855 \, J \, g^{-1} = 855000 \, J = 8.55 \times 10^5 \, J$$q = q_1 + q_2 = 1.4152 \times 10^5 \, J + 8.55 \times 10^5 \, J = 9.9652 \times 10^5 \, J$Rounding to the nearest value,we get $9.97 \times 10^5 \, J$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

Medium

The quantity of heat (in $J$) required to raise the temperature of $1.0 \, kg$ of ethanol from $293.45 \, K$ to the boiling point and then change the liquid to vapor at that temperature is closest to
[Given,boiling point of ethanol $351.45 \, K$. Specific heat capacity of liquid ethanol $2.44 \, J \, g^{-1} \, K^{-1}$. Latent heat of vaporisation of ethanol $855 \, J \, g^{-1}$ ]

KVPY 2018 All KVPY

A
$142 \times 10^2$
B
$9.97 \times 10^2$
C
$142 \times 10^5$
D
$9.97 \times 10^5$

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Mix Examples-Thermodynamics and Thermochemistry

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The heat associated with the combustion of liquid benzene at constant volume is $-3268 \ kJ \ mol^{-1}$. Calculate the change in enthalpy when this reaction occurs at $300 \ K$ $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$.

Medium

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Match the following items in List-$I$ with their corresponding expressions in List-$II$.
List-$I$ List-$II$
$A$. At constant volume the change in internal energy of a system $I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$
$B$. Isothermal irreversible change $II$. $W_{adiabatic} = \Delta U$
$C$. Isothermal reversible change $III$. $q_V = \Delta U$
$D$. Adiabatic change $IV$. $W = -p_{ex} (V_f - V_i)$
$V$. $\Delta U = \Delta H - \Delta nRT$

MediumAP EAMCET 2018

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For a diatomic ideal gas in a closed system,which of the following plots does not correctly describe the relation between various thermodynamic quantities?

DifficultJEE MAIN 2019

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Given the following thermochemical equations:
$(i) S_{(s)} + \frac{3}{2} O_{2(g)} \rightarrow SO_{3(g)} + 2x \, kcal$
$(ii) SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow SO_{3(g)} + y \, kcal$
Find the heat of formation of $SO_{2(g)}$.

Medium

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Calculate the difference between $\Delta H$ and $\Delta U$ for the following reaction at $25^{\circ} C$:
$C_2H_{6(g)} + 3.5O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$
(Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$) (in $kJ$)

MediumMHT CET 2021

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List-$I$	List-$II$
$A$. At constant volume the change in internal energy of a system	$I$. $W = -2.303 nRT \log \frac{V_f}{V_i}$
$B$. Isothermal irreversible change	$II$. $W_{adiabatic} = \Delta U$
$C$. Isothermal reversible change	$III$. $q_V = \Delta U$
$D$. Adiabatic change	$IV$. $W = -p_{ex} (V_f - V_i)$
	$V$. $\Delta U = \Delta H - \Delta nRT$

Similar Questions

The heat associated with the combustion of liquid benzene at constant volume is $-3268 \ kJ \ mol^{-1}$. Calculate the change in enthalpy when this reaction occurs at $300 \ K$ $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$.

For a diatomic ideal gas in a closed system,which of the following plots does not correctly describe the relation between various thermodynamic quantities?

Given the following thermochemical equations:$(i) S_{(s)} + \frac{3}{2} O_{2(g)} \rightarrow SO_{3(g)} + 2x \, kcal$$(ii) SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow SO_{3(g)} + y \, kcal$Find the heat of formation of $SO_{2(g)}$.

Calculate the difference between $\Delta H$ and $\Delta U$ for the following reaction at $25^{\circ} C$:$C_2H_{6(g)} + 3.5O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$(Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$) (in $kJ$)

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Given the following thermochemical equations:
$(i) S_{(s)} + \frac{3}{2} O_{2(g)} \rightarrow SO_{3(g)} + 2x \, kcal$
$(ii) SO_{2(g)} + \frac{1}{2} O_{2(g)} \rightarrow SO_{3(g)} + y \, kcal$
Find the heat of formation of $SO_{2(g)}$.

Calculate the difference between $\Delta H$ and $\Delta U$ for the following reaction at $25^{\circ} C$:
$C_2H_{6(g)} + 3.5O_{2(g)} \rightarrow 2CO_{2(g)} + 3H_2O_{(l)}$
(Given: $R = 8.314 \ J \ K^{-1} \ mol^{-1}$) (in $kJ$)