Thermodynamics

Calculate $\triangle G^\circ$ for reaction,$\text{CH}_{4(g)} + \text{H}_{2(g)} \rightarrow \text{C}_2\text{H}_{6(g)}$ ($K_p = 2 \times 10^{17}$, $R = 8.314\ \text{JK}^{-1}\text{mol}^{-1}$)

Identify the law for the statement "Overall the enthalpy change for a reaction is equal to sum of enthalpy changes of individual steps in the reaction"

If $2$ mole of an ideal gas expand isothermally and reversibly at $27^\circ$C from 1 $\text{dm}^3$ to $1\ \text{m}^3$ calculate work done? $[R = 8.314\ \text{J K}^{-1}\text{mol}^{-1}]$

Which of the following processes exhibits the decrease in internal energy of a system?

Calculate the change in internal energy if an ideal gas expands from $0.5\ \text{dm}^3$ to $3.5\ \text{dm}^3$ at constant pressure 2 bar by absorbing 1800 J heat energy.

The enthalpy of combustion of C, $\text{H}_2$, and $\text{CH}_4$ are $-390$, $-285$ and $-890$ kJ/mol. Find the enthalpy of formation of methane.

An ideal gas expands from initial volume $5\ \text{dm}^3$ to $15\ \text{dm}^3$ against a constant external pressure of $2$ atm. What is the work done by the gas ?

A gas absorbs $120$ J of heat and expands by $300 \times 10^{-6}\ \text{m}^3$ against a constant external pressure of $2 \times 10^5\ \text{Nm}^{-2}$. What will be the change in internal energy of the system ?

Identify from following, the relation between standard free energy change in a reaction and equilibrium constant $K_c$.

Which from following is NOT a state function ?

Calculate the work done for the following reaction at $27\,^\circ\text{C}$$\text{C}_2\text{H}_{4(g)} + \text{H}_{2(g)} \longrightarrow \text{C}_2\text{H}_{6(g)}$ ($R = 8.314\,\text{JK}^{-1}\text{mol}^{-1}$)

Calculate standard Gibbs energy for any gaseous reaction if values of $K_p$ and $R$ respectively are $3.5 \times 10^{17}$ ; $8.314\,\text{JK}^{-1}\text{mol}^{-1}$

Which from following is correct expression of first law of thermodynamics for isothermal process?

For a certain reaction, $\Delta\text{H}^\circ = 40\ \text{kJ}$ and $\Delta\text{S}^\circ = 80\ \text{JK}^{-1}$. Find the temperature so that $\Delta\text{G}^\circ = 0$

Calculate $\Delta\text{H}$ for the following reaction at $300\ \text{K}$$2\text{C}_{(s)} + 3\text{H}_{2(g)} \longrightarrow \text{C}_2\text{H}_{6(g)}$ if $\Delta\text{U}$ for the reaction is $-80\ \text{kJ}$ ($\text{R} = 8.314\ \text{JK}^{-...

Calculate the standard enthalpy change for the following reaction,$2\text{C}_2\text{H}_6\text{(g)} + 7\text{O}_2\text{(g)} \longrightarrow 4\text{CO}_2\text{(g)} + 6\text{H}_2\text{O}\text{(l)}$Given, $\Delta_f H^\circ(\text{C}_2\text{H}_6)...

Which of the following is the correct expression of the first law of thermodynamics for adiabatic processes ?

1 mole of an ideal gas is compressed isothermally and reversibly from initial pressure $x$ kPa to final pressure $2x$ kPa at 300 K. Find the work done $(R = 8.314\ \text{J K}^{-1}\text{mol}^{-1})$

At $25\ ^\circ\text{C}$ standard enthalpy of combustion of $\text{H}_2$, Cyclohexene and cyclohexane are -241, -3800 and -3920 kJ $\text{mol}^{-1}$ respectively. What is the heat of hydrogenation of cyclohexene?

A system is provided 50 J of heat and work done on the system is 10 J. What is change in internal energy ?

Which of the following equations is used to obtain enthalpy change of a reaction?

Which of the following processes is an endothermic ?

Calculate the standard enthalpy of combustion of carbon monoxide if$\Delta_f H^\circ (\text{CO}) = -110 \text{ kJ mol}^{-1}$$\Delta_f H^\circ (\text{CO}_2) = -393 \text{ kJ mol}^{-1}$

Calculate the quantity of heat released from system when 2 moles of and ideal gas compressed isothermally from volume $25 \text{ dm}^3$ to $10 \text{ dm}^3$ at constant external pressure 4 bar.

Which of the following relations is correct for a reaction $\text{S}_{(s)} + \text{O}_{2(g)} \rightarrow \text{SO}_{2(g)}$ ?

In a particular reaction, 4 kJ heat is released by the system and 12 kJ work done on the system. Calculate the $\Delta H$ and $\Delta U$.

What is the change in entropy of surrounding for the reaction,$\text{H}_{2(g)} + 1/2\ \text{O}_{2(g)} \rightarrow \text{H}_2\text{O}_{(l)}$at 298 K if standard enthalpy of formation of water is $-286$ kJ ?

Identify the process that proceeds with no heat exchange between system and surrounding.

Calculate the enthalpy change when 6 g. $\text{CO(g)}$ reacts with sufficient $\text{NO}_2\text{(g)}$ according to the following reaction$4\,\text{CO(g)} + 2\,\text{NO}_2\text{(g)} \rightarrow 4\,\text{CO}_2\text{(g)} + 2\text{N}_2\text{(g)...

The heat of combustion of carbon to $\text{CO}_2$ is $-393.5\ \text{kJ/mol}$. The heat released upon formation of 35.2 g of $\text{CO}_2$ from carbon and oxygen gas is

Which of the following properties of a system depends upon the amount of matter and path?

Which of the following processes has $\Delta S$ negative?

$\text{C}_2\text{H}_5\text{OH}(l) + 3\text{O}_2(g) \rightarrow 2\text{CO}_2(g) + 3\text{H}_2\text{O}(l)$The value of enthalpy change ($\Delta H$) for above reaction at $27\,^\circ\text{C}$ is $-1366.5$ kJ $\text{mol}^{-1}$. Then value of in...

Find $\Delta n$ when 1 mol of each $\text{NH}_{3(g)}$ and $\text{HCl}_{(g)}$, reacts to form solid $\text{NH}_4\text{Cl}$.

For a reaction to be spontaneous at all temperatures, the values of enthalpy change and entropy change should be

For a certain reaction, $\Delta H^0$ is $-345$ kJ and $\Delta S^0$ is $-123\ \text{JK}^{-1}$. At what temperature the change over from spontaneous to nonspontaneous will occur?

Calculate the enthalpy change of the reaction,$\text{H}_2\text{(g)} + \text{Cl}_2\text{(g)} \rightarrow 2\text{HCl(g)}$if bond energies (kJ mol$^{-1}$):H–H = 436, Cl–Cl = 242, H–Cl = 431

For a certain reaction $\Delta H = -50$ kJ and $\Delta S = -100$ J/K find the temperature so that the reaction is spontaneous.

In which of the following processes the internal energy of system remain constant?

A gas expands from a volume of $1$ dm$^3$ to $1.25$ dm$^3$ under a pressure of $1$ bar. Find the change in internal energy if $150$ J of heat is supplied to the system.

The enthalpy of combustion of cyclohexane, cyclohexene and $\text{H}_2$ are respectively $-3920, -3800$ and $-241$ KJ mol$^{-1}$. The enthalpy of hydrogenation of cyclohexene is

Which of the following processes exhibits, $\Delta U = 0$?

Calculate the work done when $1$ mole of an ideal gas is expanded reversibly and isothermally from initial pressure $10$ bar to final pressure $1$ bar at constant temperature $300$ K. [$R = 8.314 \text{ J K}^{-1} \text{ mol}^{-1}$]

Calculate the enthalpy change for the following reaction, using given bond energy (kJ/mol)(C-H = $414$, H-O = $463$, H-Cl = $431$, C-Cl = $326$ and C-O = $335$)$\text{CH}_3\text{OH}_{(g)} + \text{HCl}_{(g)} \rightarrow \text{CH}_3\text{Cl}_...

$200$ mL of ethylene gas and $150$ mL of HCl gas were allowed to react at $1$ bar. Pressure to form gaseous ethyl chloride. What is the work done during the reaction?

The bond dissociation enthalpy of $\text{H}_2$, $\text{Cl}_2$ and HCl are $434$, $242$ and $431$ kJ $\text{mol}^{-1}$ respectively. Calculate the enthalpy of formation of HCl.

The equilibrium constant for a reaction is $100$. What will be the value of standard Gibbs energy change at $298$ K ? ($R = 8.314$ J $\text{K}^{-1}\text{mol}^{-1}$)

Calculate the work done in the oxidation of one mole $\mathrm{HCl}_{(\mathrm{g})}$ at $27^{\circ} \mathrm{C}$, according to reaction.
$$ \begin{aligned} & 4 \mathrm{HCl}_{(\mathrm{g})}+\mathrm{O}_{2(\mathrm{~g})} \longrightarrow 2 \mathrm{C...

Which from following is an example of an intensive property of the system?

For a certain reaction $\Delta \mathrm{H}=-225 \mathrm{~kJ}$ and $\Delta S=-150 \mathrm{JK}^{-1}$. Find the temperature so that $\Delta G$ is zero.