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 | $\Delta H \ (kJ/mol)$ |
|---|---|
| $I. \ \frac{1}{2} A \rightarrow B$ | $+150$ |
| $II. \ 3B \rightarrow 2C + D$ | $-125$ |
| $III. \ E + A \rightarrow 2D$ | $+350$ |
For $B + D \rightarrow E + 2C, \Delta H$ will be ............. $kJ/mol$
- A$525$
- B$-175$
- C$-325$
- D$325$
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Similar Questions
Given that:
$2C_{(s)} + 2O_{2(g)} \to 2CO_{2(g)}$; $\Delta H = -787 \ kJ$
$H_{2(g)} + \frac{1}{2} O_{2(g)} \to H_2O_{(l)}$; $\Delta H = -286 \ kJ$
$C_2H_{2(g)} + \frac{5}{2} O_{2(g)} \to 2CO_{2(g)} + H_2O_{(l)}$; $\Delta H = -1301 \ kJ$
Calculate the heat of formation of acetylene $(C_2H_{2(g)})$ in $kJ$.
$2C_{(s)} + 2O_{2(g)} \to 2CO_{2(g)}$; $\Delta H = -787 \ kJ$
$H_{2(g)} + \frac{1}{2} O_{2(g)} \to H_2O_{(l)}$; $\Delta H = -286 \ kJ$
$C_2H_{2(g)} + \frac{5}{2} O_{2(g)} \to 2CO_{2(g)} + H_2O_{(l)}$; $\Delta H = -1301 \ kJ$
Calculate the heat of formation of acetylene $(C_2H_{2(g)})$ in $kJ$.
Medium
View SolutionWhen $10 \ g$ of methane is completely burnt in oxygen, the heat evolved is $560 \ kJ$. What is the heat of combustion (in $kJ \ mol^{-1}$) of methane?
$H_{2(g)} + \frac{1}{2}O_{2(g)} \to H_2O_{(l)}$; $\Delta H$ at $298 \ K = -285.8 \ kJ$. The molar enthalpy of vaporization of water at $1 \ atm$ and $25^{\circ}C$ is $44 \ kJ$. The standard enthalpy of formation of $1 \ mole$ of water vapor at $25^{\circ}C$ is $...... \ kJ$. (in $.8$)
Medium
View SolutionEnthalpies of formation of $CCl_{4(g)}$,$H_2O_{(g)}$,$CO_{2(g)}$ and $HCl_{(g)}$ are $-105$,$-242$,$-394$ and $-92 \ kJ \ mol^{-1}$ respectively. The magnitude of enthalpy of the reaction given below is $...... \ kJ \ mol^{-1}$ (nearest integer): $CCl_{4(g)} + 2H_2O_{(g)} \rightarrow CO_{2(g)} + 4HCl_{(g)}$
At $25^{\circ} C$ and $1 \ atm$ pressure,the enthalpies of combustion are as given below:
Substance $H_{2(g)}$ $C_{\text{(graphite)}}$ $C_{2}H_{6(g)}$ $\Delta_{c}H^{\Theta} / (kJ \ mol^{-1})$ $-286.0$ $-394.0$ $-1560.0$
The enthalpy of formation of ethane is ........ .
| Substance | $H_{2(g)}$ | $C_{\text{(graphite)}}$ | $C_{2}H_{6(g)}$ |
| $\Delta_{c}H^{\Theta} / (kJ \ mol^{-1})$ | $-286.0$ | $-394.0$ | $-1560.0$ |
The enthalpy of formation of ethane is ........ .
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