Given that the bond energy of hydrogen-hydrog | vedclass

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

Question

(A) The heat of reaction $\Delta H$ is calculated using the formula: $\Delta H = \sum 	ext{Bond Energy of Reactants} - \sum 	ext{Bond Energy of Prod

Vedclass · Accepted Answer

$-488$

Vedclass · Answer

(A) The heat of reaction $\Delta H$ is calculated using the formula: $\Delta H = \sum 	ext{Bond Energy of Reactants} - \sum 	ext{Bond Energy of Products}$.For the reaction $2H_2 + O_2 \longrightarrow 2H_2O$,the bonds broken are $2 	imes (H-H)$ and $1 	imes (O=O)$.Total energy required to break bonds = $2 	imes 436 + 496 = 872 + 496 = 1368 \ kJ/mol$.The bonds formed are $4 	imes (O-H)$ (since there are two $H_2O$ molecules,each with two $O-H$ bonds).Total energy released during bond formation = $4 	imes 464 = 1856 \ kJ/mol$.$\Delta H = 1368 - 1856 = -488 \ kJ/mol$.

Given that the bond energy of hydrogen-hydrogen bond is $436 \ kJ/mol$,that of hydrogen-oxygen bond is $464 \ kJ/mol$,and those in oxygen molecules $496 \ kJ/mol$,what is the approximate heat of reaction for $2H_2 + O_2 \longrightarrow 2H_2O$ ? .....$kJ/mol$

Similar Questions

The average $C-H$ bond energy is $416 \ kJ \ mol^{-1}$. Which of the following equations correctly represents the bond dissociation of $CH_4$?

The enthalpy of the reaction,$H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(g)}$ is $\Delta H_1$ and that of $H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}$ is $\Delta H_2$. Then:

$H_2 + Cl_2 \longrightarrow 2HCl$ ; $\Delta H = -x \ kJ$
$NaCl + H_2SO_4 \longrightarrow NaHSO_4 + HCl$ ; $\Delta H = -y \ kJ$
$2H_2O + 2Cl_2 \longrightarrow 4HCl + O_2$ ; $\Delta H = -z \ kJ$
From the above equations,the value of $\Delta H_f$ of $HCl$ is:

Which of the following values of heat of formation indicates that the product is least stable in $kcal$?

Find the bond enthalpy of $N-H$ bond in ammonia by using the change in enthalpy for the reaction given below: $N_{2(g)} + 3H_{2(g)} \to 2NH_{3(g)}$; $\Delta H = -23 \ kcal$. Given bond energies: $N \equiv N = 226 \ kcal/mol$,$H-H = 103 \ kcal/mol$.

Vedclass Test Series

Exam Paper Generator

Online Exam Module