Thermodynamics practice · Mixed difficulty

Identify the correct statement from the
following is a chemical reaction.

In biological cells that have a plentiful supply of $\mathrm{O}_2,$ glucose is oxidized completely to $\mathrm{CO}_2$ and $\mathrm{H}_2 \mathrm{O}$ by a process called aerobic oxidation. Muscle cells may be deprived of $\mathrm{O}_2$ during vigorous exercise and in that case, one molecule of glucose is converted to two molecules of lactic acid, $\mathrm{CH}_3 \mathrm{CH}(\mathrm{OH}) \mathrm{COOH},$ by a process called anaerobic glycolysis.

$\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6(\mathrm{s})+6 \mathrm{O}_2(\mathrm{g}) \rightarrow 6 \mathrm{CO}_2(\mathrm{g})+6 \mathrm{H}_2 \mathrm{O}({l}) ; \Delta H^{\circ}=-2880 \mathrm{~kJ} / \mathrm{mol}$

$\mathrm{C}_6 \mathrm{H}_{12} \mathrm{O}_6(\mathrm{s}) \rightarrow 2 \mathrm{CH}_3 \mathrm{CH}(\mathrm{OH}) \mathrm{COOH}(\mathrm{s}) ; \Delta H^{\circ}=+2530 \mathrm{~kJ} / \mathrm{mol}$

Which of the following statements is true regarding aerobic oxidation and anaerobic glycolysis with respect to energy change as heat?

Two moles of an ideal gas $\left(C_{v, m}=\frac{5}{2} R\right)$ was compressed adiabatically against constant pressure of $2 \mathrm{~atm},$ which was initially at $350 \mathrm{~K}$ and $1 \mathrm{~atm}.$ The work done on the gas in this process is

The temperature coefficient of e.m.f. of a cell can be given by:

In the following reactions,

I. $30 \mathrm{~mL}$ of $0.1 \mathrm{~M} \mathrm{~Ba}(\mathrm{OH})_2(a q)+30 \mathrm{~mL}$ of $0.1 \mathrm{~M} \mathrm{~H}_2 \mathrm{SO}_4(\mathrm{aq})$, rise in temperature $=\Delta T_1$

II. $90 \mathrm{~mL}$ of $0.1 \mathrm{~M} \mathrm{~Ba}(\mathrm{OH})_2(\mathrm{aq})+90 \mathrm{~mL}$ of $0.1 \mathrm{~M} \mathrm{~H}_2 \mathrm{SO}_4(a q)$, rise in temperature $=\Delta T_2$. Thus,

Following reaction occurs in an automobile $2{C_8}{H_{18}}(g) + 25\,{O_2}(g) \to 16\,C{O_2}(g) + 18{H_2}O(g)$ The sign of $\Delta H,\,\Delta S\mathrm{ }\,\mathrm{and}\,\,\mathrm{ }\Delta G$ would be

In which of the following changes entropy
decreases ?

The total heat content of a system at constant pressure is

An ideal gas was subjected to a reversible adiabatic expansion then its initial volume was restored by reversible, isothermal compression. If ' $q$ ' denotes the heat added to the system and $w$ the work done on the system for the overall process then

If heat of dissociation of ${CHCl}_2{COOH}$ is $0.7 \mathrm{~Kcal} / \mathrm{mol}$ then $\Delta {H}$ for the reaction:

${CHCl}_2 {COOH}+{KOH} \rightarrow {CHCl}_2 {COOK}+{H}_2 {O}$

Assertion : Born-Haber cycle is based on Hess's law.

Reason : Lattice enthalpy can be calculated by Born Haber cycle.

$\begin{aligned} & \Delta H_f^{\circ}\left(\mathrm{NO}_2\right)=33.84 \mathrm{~kJ} \mathrm{~mol}^{-1} \\ & \Delta H_f^{\circ}\left(\mathrm{N}_2 \mathrm{O}_4\right)=9.66 \mathrm{~kJ} \mathrm{~mol}^{-1} \end{aligned}$

hence, dimerisation of $\mathrm{NO}_2$ forming $\mathrm{N}_2 \mathrm{O}_4$ is

The enthalpy of vaporization of substance is $840 \mathrm{~J-} \mathrm{mol}^{-1}$ and its boiling point is $-173^{\circ} \mathrm{C}$. Its entropy of vaporization is:

Assertion :- At constant pressure of the change $\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})$ work done is negative.

Reason :- During phase transition work done is always negative.

The work done by a weightless piston in causing an expansion ∆V (at constant temperature), when the opposing pressure, P is variable, is given by:

What is the entropy change $(in J{K^{ - 1}}mo{l^{ - 1}})$ when one mole of ice is converted into water at 0℃? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol^(-1) at 0℃)

Assertion : The mass and volume of a substance are the extensive properties and are proportional to each other.

Reason : The ratio of mass of a sample to its volume is an intensive property.

Work done by a sample of an ideal gas in a process ${A}$ is double the work done in another process ${B}.$ The temperature rises through the same amount in the two processes. If $C_{{A}}$ and $C_{{B}}$ are the molar heat capacities for the two processes, then

The standard state Gibbs free energies of formation of $C$ (graphite) and C (diamond) at $T=298 {~K}$ are

$\begin{aligned} & \Delta_f G^{\circ}[{C} \text { (graphite) }]=0 {~kJ} {~mol}^{-1} \\ & \Delta_f G^{\circ}[{C} \text { (diamond) }]=2.9 {~kJ} {~mol}^{-1} \end{aligned}$

The standard state means that the pressure should be 1 bar, and substance should be pure at a given temperature. The conversion of graphite [C(graphite)] to diamond $\left[C\right.$ (diamond)] reduces its volume by $2 \times 10^{-6} {~m}^3 {~mol}^{-1}$. If ${C}$ (graphite) is converted to ${C}$ (diamond) isothermally at ${T}$ $=298 {~K}$, the pressure at which ${C}$ (graphite) is in equilibrium with ${C}$ (diamond), is :

$[\text{Useful information:}$ $1 {~J}=1 {~kg} {~m}^2 {~s}^{-2}$;
$\left.1 {~Pa}=1 {~kg} {~m}^{-1} {~s}^{-2} ; 1 {bar}=10^5 {~Pa}\right]$

$\mathrm{C}_{\mathrm{v}}$ for monatomic gas is

Read the following statements carefully and choose the correct option

(i) The state of the system is specified by state functions or state variables.

(ii) Variables like $\mathrm{P}, \mathrm{V}$ and $\mathrm{T}$ are called state variables or state functions

(iii) Their values depend only on the state of the system and not on how it is reached.

The heat of neutralization of ${NaOH}$ with ${HCl}$ is $57.3 {~kJ}$ and with ${HCN}$ is $12.1 {~kJ}$. The heat of ionization of ${HCN}$ is

For which of the following elements, the standard enthalpy is not zero.

Which selection correctly shows units for specific heat capacity?

Assertion (A): Heat of neutralisation is always less than zero.

Reason (R): Neutralisation involves reaction between an acid and a base.

${Na}(\mathrm{s}) \rightarrow {Na}(\mathrm{g})$, the heat of reaction is called as

Given, $\mathrm{H}_2 \mathrm{O}(l) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g}) ; \Delta \mathrm{H}_1=+43.7 \mathrm{~kJ}$ $\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(l) ; \Delta \mathrm{H}_2=+6.05 \mathrm{~kJ}$ Calculate the enthalpy of sublimation of ice.

Enthalpy change in the formation of $\mathrm{Cl}^{+} \mathrm{Cl}^{-}$(imaginary) lattice from $\mathrm{Cl}_2$ based on following data is $\mathrm{Cl}-\mathrm{Cl}$ bond energy= $x_1$, ionisation energy of $\mathrm{Cl}=x_2$ electron affinity of $\mathrm{Cl}=x_3$, lattice energy of $\mathrm{Cl}^{+} \mathrm{Cl}^{-}=x_4$

Assertion : Heat absorbed in a reaction at constant temperature and constant volume is $-\Delta G$.

Reason : $\Delta G$ should be negative for the reaction to be spontaneous.

At $27^{\circ} \mathrm{C}$ latent heat of fusion of a compound is $2930 \mathrm{~J} / \mathrm{mol}$. Entropy change is