Thermodynamics practice · Mixed difficulty

Select the correct set of statements considering initial state to be same and final state at same volume in case of comparison.

(I) Magnitude of Work done on the surrounding in case of infinite step expansion is more than single stage expansion for an isothermal process.

(II) Irreversible work is always greater than reversible work for an isothermal process. (with sign)

(III) On an ideal gas in case of single stage expansion and compression, system as well as surrounding are restored back to their original states.

(IV) If gas in thermodynamic equilibrium is taken from state A to state B, by four successive single stage expansions. Then we can plot maximum 4 points on the $\mathrm{P}-\mathrm{V}$ indicator diagram.

The values of ∆H and ∆S for the reaction. ${C_{\left( {\mathrm{graphite}} \right)}} + \mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) \to 2\mathrm{CO}\left( \mathrm{g} \right)$ Are 170 kJ and 170 $\mathrm{J}{\mathrm{K}^{ - 1}}$ respectively. this reaction will be spontaneous at:

Internal energy of an ideal gas depends on:

A carnot engine operates between temperature T and 400 K (T>400 K). If efficiency of engine is 25%, the temperature T is:

5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K. If ${C_V} = 28\mathrm{ }\,\,J{K^{ - 1}}\mathrm{ }mo{l^{ - 1}},$ calculate $\Delta U\mathrm{ }$ and $\Delta pV$ for this process, $(R = 8.0\mathrm{ }\,J{K^{ - 1}}\mathrm{ }mo{l^{ - 1}})$

If a man takes a diet which gives him energy equal to $9500 \mathrm{~kJ}$ per day and he expands energy all forms to a total of $12000 \mathrm{~kJ}$ per day, what is the change in internal energy per day? If the energy lost was stored as sucrose (1632 kJ per $100 \mathrm{~g}$ ), how many days should it take to loss $1 \mathrm{~kg}$ ? Ignore the water loss.

The amount of heat measured for a reaction in a bomb calorimeter is

Entropy decreases during:

A container has hydrogen and oxygen mixture in ratio of 4∶1 by weight, then:

STATEMENT-1 : The standard free energy changes of all spontaneously occuring reactions are negative.

STATEMENT-2 : The standard free energies of the elements in their standard states at 1 bar and 298 K are taken as zero.

Which one of the following is used to remove most of plutonium from spent nuclear fuel?

For which process energy will be absorbed?

Which is correct about the heat of combustion?

Assertion: When ideal gas expand from $P_1, V_1, T_1$ to $P_2, V_2, T_2$ in multiple steps, work done is high where number of steps are high.
Reason: Work is path function.

If the pressure and density of a diatomic gas $(\gamma=7 / 5)$ in adiabatic process changes from $(P, d)$ to $\left(P^{\prime}, d^{\prime}\right)$, where $p / p^{\prime}$ is 32 then $\mathrm{d}$ '/ $\mathrm{d}$ is $32 x$, find $x$ ?

Minimum work is obtained when 1 kg of … gas expanded under 500 kPa to 200 kPa pressure at 0℃.

The normal boiling point and $\Delta {H}_{\text {vap }}$ of a liquid ' ${X}$ ' are $400 {~K}$ and $40 {~kJ} {~mol}^{-1}$ respectively. Assuming $\Delta {H}_{\text {vap }}$ to be constant, which of the following is correct?
(I) $\Delta {S}_{\text {vap }}>100 {JK}^{-1} {~mol}^{-1}$ at $400 {~K}$ and $0.5 {~atm}$
(II) $\Delta {S}_{\text {vap }} < 100 {JK}^{-1} {~mol}^{-1}$ at $400 {~K}$ and $1 {~atm}$
(III) $\Delta {S}_{\text {vap }} < 100 {JK}^{-1} {~mol}^{-1}$ at $400 {~K}$ and $2 {~atm}$
(IV) $\Delta {S}_{\text {vap }}=100 {JK}^{-1} {~mol}^{-1}$ at $400 {~K}$ and $1 {~atm}$

The variation of equilibrium constant with temperature is given below:
$\begin{array}{cccccccccccccccccccc} {\mathrm{Temperature}}&{\mathrm{Equilibrium\,\, constant}}\\ {{T_1} = {{25}^ \circ }C}&{{K_1} = 10}\\ {{T_2} = {{100}^ \circ }C}&{{K_2} = 100} \end{array}$
The values of $\Delta \mathrm{H}^\circ ,\Delta \mathrm{G}^\circ \,\,\,\,\mathrm{at }\,\,{\mathrm{T}_\mathrm{1}}\mathrm{ }\,\mathrm{and}\,\,\mathrm{ }\Delta G^\circ \,\,\mathrm{ at}\,\,\mathrm{ }{\mathrm{T}_2}\mathrm{ }\,\,\mathrm{(in}\,\,\mathrm{ kJ}\,\,\mathrm{ mo}{\mathrm{l}^{ - 1}})$ respectively, are close to [Use $R\mathrm{ } = \mathrm{ }8.314\mathrm{ }J{K^{ - 1}}mo{l^{ - 1}}]$

Specific heat is defined as:

${H_2}$ (g)+Cl(g)=2HCl(g); ∆H(298 K)=22.06 kcal. For this reaction, ∆U is equal to:

48 g of C (diamond) on complete combustion evolves 1584 kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energies required for the process
(i)C (graphite) → C(gas)
(ii)C (diamond) → C(gas)are:

The word standard in molar enthalpy change implies

The heat of combustion of ethanol determined by a bomb calorimeter is - 670.48 kcal$mo{l^{ - 1}}$ at ${25^0}C$.What is ∆U at ${25^0}C$ for the following reaction? ${\mathrm{C}_2}{\mathrm{H}_5}\mathrm{OH}\left( l \right) + \frac{7}{2}{\mathrm{O}_2}\left( \mathrm{g} \right) \to 2\mathrm{C}{\mathrm{O}_2}\left( \mathrm{g} \right) + 3{\mathrm{H}_2}\mathrm{O}\left( \mathrm{g} \right)$

∆n values in ∆H= ∆U+ ∆nRT may have:

For the reaction $CC{l_{4\left( g \right)}} + 2{H_2}{O_{\left( g \right)}} \to C{O_{2\left( g \right)}} + 4HC{l_{\left( g \right)}}$ at constant temperature , $\Delta H - \Delta E$ is

Gibbs energy G, enthalpy H and entropy S are related by:

When one mole of an ideal gas is compressed to half its initial volume and simultaneously heated to twice in initial temperature, the change in entropy $(\Delta S)$ is

The total heat content of a system at constant pressure is

Which of the following is correct for a reaction to be spontaneous?

Entropy change of vaporisation at constant pressure is given by: