(B) To obtain the target reaction $B + D \rightarrow E + 2C$,we manipulate the given equations:$1. \ 2 \times (I): A \rightarrow 2B, \Delta H = 2 \tim

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(B) To obtain the target reaction $B + D \rightarrow E + 2C$,we manipulate the given equations:$1. \ 2 \times (I): A \rightarrow 2B, \Delta H = 2 \times 150 = 300 \ kJ/mol$$2. \ (II): 3B \rightarrow 2C + D, \Delta H = -125 \ kJ/mol$$3. \ -(III): 2D \rightarrow E + A, \Delta H = -350 \ kJ/mol$Adding these equations:$(A + 3B + 2D) \rightarrow (2B + 2C + D + E + A)$Simplifying by canceling common terms ($A$ and $2B$ and $D$ from both sides):$B + D \rightarrow E + 2C$$\Delta H = 300 - 125 - 350 = -175 \ kJ/mol$

Class 11 Chemistry Thermodynamics Heat of reaction, Bond energy and Hess law

Medium

Consider the following processes:

Process $\Delta H \ (kJ/mol)$

$I. \ \frac{1}{2} A \rightarrow B$ $+150$

$II. \ 3B \rightarrow 2C + D$ $-125$

$III. \ E + A \rightarrow 2D$ $+350$

For $B + D \rightarrow E + 2C, \Delta H$ will be ............. $kJ/mol$

Process	$\Delta H \ (kJ/mol)$
$I. \ \frac{1}{2} A \rightarrow B$	$+150$
$II. \ 3B \rightarrow 2C + D$	$-125$
$III. \ E + A \rightarrow 2D$	$+350$

AIPMT 2011 All AIPMT

A
$525$
B
$-175$
C
$-325$
D
$325$

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

Thermodynamics

Subtopic

Heat of reaction, Bond energy and Hess law

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AIPMT 2011 Paper All AIPMT years →

Given the reactions:
$C + \frac{1}{2}O_2 \to CO : \Delta H = -12 \ kJ$
$CO + \frac{1}{2}O_2 \to CO_2 : \Delta H = -10 \ kJ$
For the reaction $C + O_2 \to CO_2 : \Delta H = x \ kJ$,the value of $x$ is: (in $kJ$)

Medium

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Match the following allotropes of carbon with their standard enthalpy of formation $(\Delta_f H^{\Theta})$:
Allotrope $\Delta_f H^{\Theta}$
$i$. Graphite $b$. $0 \ kJ/mol$
$ii$. Diamond $c$. $1.90 \ kJ/mol$
$iii$. Fullerene $a$. $38.1 \ kJ/mol$

Easy

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$C_{(diamond)} + O_2 \to CO_2; \Delta H = -395.3 \ kJ/mole$
$C_{(graphite)} + O_2 \to CO_2; \Delta H = -393.4 \ kJ/mole$
$C_{(graphite)} \to C_{(diamond)}; \Delta H = ?$

Medium

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Enthalpy change for a reaction does not depend upon

EasyAIEEE 2003

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The heat of combustion of methane is $-809 \, kJ \, mol^{-1}$. What is the calorific value of methane in $kJ \, g^{-1}$?

Medium

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Allotrope	$\Delta_f H^{\Theta}$
$i$. Graphite	$b$. $0 \ kJ/mol$
$ii$. Diamond	$c$. $1.90 \ kJ/mol$
$iii$. Fullerene	$a$. $38.1 \ kJ/mol$

Consider the following processes: Process $\Delta H \ (kJ/mol)$ $I. \ \frac{1}{2} A \rightarrow B$ $+150$ $II. \ 3B \rightarrow 2C + D$ $-125$ $III. \ E + A \rightarrow 2D$ $+350$ For $B + D \rightarrow E + 2C, \Delta H$ will be ............. $kJ/mol$

Similar Questions

Given the reactions: $C + \frac{1}{2}O_2 \to CO : \Delta H = -12 \ kJ$ $CO + \frac{1}{2}O_2 \to CO_2 : \Delta H = -10 \ kJ$ For the reaction $C + O_2 \to CO_2 : \Delta H = x \ kJ$,the value of $x$ is: (in $kJ$)

Match the following allotropes of carbon with their standard enthalpy of formation $(\Delta_f H^{\Theta})$:Allotrope$\Delta_f H^{\Theta}$$i$. Graphite$b$. $0 \ kJ/mol$$ii$. Diamond$c$. $1.90 \ kJ/mol$$iii$. Fullerene$a$. $38.1 \ kJ/mol$

$C_{(diamond)} + O_2 \to CO_2; \Delta H = -395.3 \ kJ/mole$$C_{(graphite)} + O_2 \to CO_2; \Delta H = -393.4 \ kJ/mole$$C_{(graphite)} \to C_{(diamond)}; \Delta H = ?$

Enthalpy change for a reaction does not depend upon

The heat of combustion of methane is $-809 \, kJ \, mol^{-1}$. What is the calorific value of methane in $kJ \, g^{-1}$?

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Consider the following processes:

Process $\Delta H \ (kJ/mol)$

$I. \ \frac{1}{2} A \rightarrow B$ $+150$

$II. \ 3B \rightarrow 2C + D$ $-125$

$III. \ E + A \rightarrow 2D$ $+350$

For $B + D \rightarrow E + 2C, \Delta H$ will be ............. $kJ/mol$

Given the reactions:
$C + \frac{1}{2}O_2 \to CO : \Delta H = -12 \ kJ$
$CO + \frac{1}{2}O_2 \to CO_2 : \Delta H = -10 \ kJ$
For the reaction $C + O_2 \to CO_2 : \Delta H = x \ kJ$,the value of $x$ is: (in $kJ$)

Match the following allotropes of carbon with their standard enthalpy of formation $(\Delta_f H^{\Theta})$:
Allotrope $\Delta_f H^{\Theta}$
$i$. Graphite $b$. $0 \ kJ/mol$
$ii$. Diamond $c$. $1.90 \ kJ/mol$
$iii$. Fullerene $a$. $38.1 \ kJ/mol$

$C_{(diamond)} + O_2 \to CO_2; \Delta H = -395.3 \ kJ/mole$
$C_{(graphite)} + O_2 \to CO_2; \Delta H = -393.4 \ kJ/mole$
$C_{(graphite)} \to C_{(diamond)}; \Delta H = ?$