Difference between Internal Energy and Enthalpy

Q.

What Is The Significance Of The Thermodynamic Enthalpy?

Q. Which is not the correct relation between enthalpy $\Delta H$ and intrinsic energy $\Delta E$

1. $\Delta H=\Delta E+P\Delta V$
2. $\Delta H=\Delta E+nRT$
3. $\Delta H=\Delta E-P\Delta V$
4. $\Delta E=\Delta H-P\Delta V$

Q. $1$ mol of an ideal gas for which $C_v=\frac{3}{2}R$ is heated reversibly at a constant pressure of $1$ atm from $25{}^{o}C$ to $100{}^{o}C$. The $△H$ is:
Given: $R=1.987\text{cal}$

1. $3.775\text{cal}$
2. $37.256\text{cal}$
3. $372.56\text{cal}$
4. $3725.6\text{cal}$

Q. For the reaction, $C_{\left(s\right)}+O_{2\left(g\right)}\to C{O}_{2\left(g\right)}$

1. $\Delta H$>$\Delta U$
2. $\Delta H$<$\Delta U$
3. $\Delta H$=$\Delta U$
4. Cannot be predicted

Q.

What is enthalpy used for?

Q.

Complete and balance the given equation :

${\mathrm{CH}}_4+{\mathrm{O}}_2\to$

Q. At constant T and P, which one of the following statements is correct for the reaction, $CO\left(g\right)+\frac{1}{2}{O}_2\left(g\right)\to C{O}_2\left(g\right)$

1. $\Delta H$ is independent of the physical state of the reactants of that compound
2. $\Delta H>\Delta E$
3. $\Delta H<\Delta E$
4. $\Delta H=\Delta E$

Q. $(\Delta H-\Delta U)$ in J/mol for the formation of carbon monoxide $\left(CO\right)$ from its elements at $300\text{K}$ is:$R=\frac{25}{3}\text{J/Kmol}$

Q.

The heat of combustion of ethylene at ${18}^{\circ }C$ and at constant volume is -335.8 K cal when water is obtained in liquid state. What is the heat of combustion at constant pressure and at ${18}^{\circ }C$.

1. -337 k cal

2. 337 k cal

3. 237 k cal

4. -237k cal

Q. Given the following standard heat of reactions :
(i) heat of formation of water = $-68.3\text{kcal}$
(ii) heat of combustion of acetylene = $-310.6\text{kcal}$
(iii) heat of combustion of ethylene = $-337.2\text{kcal}$
Which of the following option(s) is / are correct for the hydrogenation of acetylene at constant volume $\left({27}^{\circ }\text{C}\right)$?
(Given, $R=2\times {10}^{-3}\text{kcal}{K}^{-1}{\text{mol}}^{-1}$)

1. Change in enthalpy of hydrogenation of acetylene is $-41.7\text{kcal}$
2. Change in internal energy of hydrogenation of acetylene is $-41.7\text{kcal}$
3. Change in enthalpy of hydrogenation of acetylene is $-41.1\text{kcal}$
4. Change in internal energy of hydrogenation of acetylene is $-41.1\text{kcal}$

Q. $3000\text{J}$ of heat is given to a gas at a constant pressure of
$P=2\times {10}^5{\text{N/m}}^2.$
If its volume increases by $10$ litres during the process, find the change in internal energy of the gas. (in Joules)

Q. $1$ mol of an ideal gas for which $C_v=\frac{3}{2}R$ is heated reversibly at a constant pressure of $1$ atm from $25{}^{o}C$ to $100{}^{o}C$. The $△H$ is:
Given: $R=1.987\text{cal}$

1. $3.775\text{cal}$
2. $37.256\text{cal}$
3. $372.56\text{cal}$
4. $3725.6\text{cal}$

Q. The value of $K_p$ for the following reaction $2H_{2}S\left(g\right)\rightleftharpoons 2H_2\left(g\right)+S_2\left(g\right)is1.2\times {10}^{-2}at{106.5}^{o}C.$ The value of $K_C$ for this reaction is

1. $1.2\times {10}^{-2}$
2. $<1.2\times {10}^{-2}$
3. 83
4. $>1.2\times {10}^{-2}$

Q. What is the relation between $\Delta H$ and $\Delta E$ in this reaction?
$C{H}_{4\left(g\right)}+2O_{2\left(g\right)}\rightleftharpoons C{O}_{2\left(g\right)}+2H_2{O}_{\left(l\right)}$

1. $\Delta H=\Delta E-RT$
2. $\Delta H=\Delta E-\frac{RT}{2}$
3. $\Delta H=\Delta E+2RT$
4. $\Delta H=\Delta E-2RT$