(A) The heat released during combustion is absorbed by the calorimeter: $q = C_V \times \Delta T$.Given $C_V = 2.5 \ kJ \ K^{-1}$ and $\Delta T = 298.

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

(A) The heat released during combustion is absorbed by the calorimeter: $q = C_V \times \Delta T$.Given $C_V = 2.5 \ kJ \ K^{-1}$ and $\Delta T = 298.45 \ K - 298.0 \ K = 0.45 \ K$.Heat released for $3.5 \ g$ of gas $= 2.5 \ kJ \ K^{-1} \times 0.45 \ K = 1.125 \ kJ$.Moles of gas $= \frac{\text{mass}}{\text{molecular weight}} = \frac{3.5 \ g}{28 \ g \ mol^{-1}} = 0.125 \ mol$.Enthalpy of combustion per mole $= \frac{\text{Heat released}}{\text{moles}} = \frac{1.125 \ kJ}{0.125 \ mol} = 9 \ kJ \ mol^{-1}$.

Class 11 Chemistry Thermodynamics Mix Examples-Thermodynamics and Thermochemistry

In a constant volume calorimeter,$3.5 \ g$ of a gas with molecular weight $28$ was burnt in excess oxygen at $298.0 \ K$. The temperature of the calorimeter was found to increase from $298.0 \ K$ to $298.45 \ K$ due to the combustion process. Given that the heat capacity of the calorimeter is $2.5 \ kJ \ K^{-1}$,the numerical value for the enthalpy of combustion of the gas in $kJ \ mol^{-1}$ is

IIT 2009 All IIT

A
$9$
B
$4$
C
$5$
D
$6$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

Thermodynamics

Subtopic

Mix Examples-Thermodynamics and Thermochemistry

Previous Year

IIT 2009 Paper All IIT years →

When $3 \ mol$ of $Ar_{(g)}$ is supplied with $229 \ J$ of heat at constant pressure,the temperature of the sample increases by $2.55 \ K$. Calculate the molar heat capacity of the gas at constant volume.

Medium

View Solution

If $100$ mole of $H_2O_2$ decomposes at $1$ bar and $300$ $K$,the work done $(kJ)$ by $50$ mole of $O_{2(g)}$ as it expands against $1$ bar pressure is............. $kJ$
$2H_2O_{2(l)} \rightleftharpoons 2H_2O_{(l)} + O_{2(g)}$
$(R = 8.3 \ J \ K^{-1} \ mol^{-1})$

DifficultJEE MAIN 2016

View Solution

$A$ 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 = $1.0 \, kcal/kg \cdot K$)

Difficult

View Solution

Which of the following is true for the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $100 ^oC$ and $1 \text{atm}$ pressure?

EasyAIIMS 1996

View Solution

Which of the following relations is correct?

Medium

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

Similar Questions

When $3 \ mol$ of $Ar_{(g)}$ is supplied with $229 \ J$ of heat at constant pressure,the temperature of the sample increases by $2.55 \ K$. Calculate the molar heat capacity of the gas at constant volume.

If $100$ mole of $H_2O_2$ decomposes at $1$ bar and $300$ $K$,the work done $(kJ)$ by $50$ mole of $O_{2(g)}$ as it expands against $1$ bar pressure is............. $kJ$$2H_2O_{2(l)} \rightleftharpoons 2H_2O_{(l)} + O_{2(g)}$$(R = 8.3 \ J \ K^{-1} \ mol^{-1})$

Which of the following is true for the reaction $H_2O_{(l)} \rightleftharpoons H_2O_{(g)}$ at $100 ^oC$ and $1 \text{atm}$ pressure?

Which of the following relations is correct?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

If $100$ mole of $H_2O_2$ decomposes at $1$ bar and $300$ $K$,the work done $(kJ)$ by $50$ mole of $O_{2(g)}$ as it expands against $1$ bar pressure is............. $kJ$
$2H_2O_{2(l)} \rightleftharpoons 2H_2O_{(l)} + O_{2(g)}$
$(R = 8.3 \ J \ K^{-1} \ mol^{-1})$