State Hess's Law of Constant Heat Summation.
(N/A) Hess's Law of Constant Heat Summation states that the total enthalpy change for a chemical reaction is the same,whether the reaction occurs in one step or in several steps. Mathematically,the total enthalpy change is the algebraic sum of the enthalpy changes of the individual steps: $\Delta H_{total} = \sum \Delta H_{steps}$.
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Similar Questions
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 $a$. $38.1 \ kJ/mol$
| 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
View SolutionGiven 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 $2H_2 + O_2 \longrightarrow 2H_2O$ ? .....$kJ/mol$
Difficult
View SolutionFind the enthalpy of formation of the $OH^-$ ion in $KJ$ at $25^\circ C$ from the following data:
$H_2O_{(l)} \to H^+_{(aq)} + OH^-_{(aq)} ; \Delta H = 57.32 \ KJ$
$H_{2(g)} + \frac{1}{2} O_{2(g)} \to H_2O_{(l)} ; \Delta H = -286.20 \ KJ$
$H_2O_{(l)} \to H^+_{(aq)} + OH^-_{(aq)} ; \Delta H = 57.32 \ KJ$
$H_{2(g)} + \frac{1}{2} O_{2(g)} \to H_2O_{(l)} ; \Delta H = -286.20 \ KJ$
Difficult
View SolutionGiven: $S + \frac{3}{2} O_2 \to SO_3 + 2x \ \text{kcal}$,$\Delta H = -2x \ \text{kcal}$ and $SO_2 + \frac{1}{2} O_2 \to SO_3 + y \ \text{kcal}$,$\Delta H = -y \ \text{kcal}$. Find the heat of formation of $SO_2$.
Difficult
View SolutionEqual volumes of molar hydrochloric acid and sulphuric acid are neutralized by dilute $NaOH$ solution and $x \ kcal$ and $y \ kcal$ of heat are liberated respectively. Which of the following is true?
MediumWBJEE 2009
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