NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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2 {MnO}_4^{-}+16 {H}^{+}+10 {Cl}^{-} \rightarrow 2 {Mn}^{2+}+5 {Cl}_2(\mathrm{g})+8 {H}_2 {O}

The above reaction is endothermic and hence, the actual temperature of the reaction vessel (isolated from the surrounding) may be different from that expected. Given that the initial temperature of the reaction vessel was used in the calculations, how would this affect the predicted value of moles of

{Cl}_2(n)

according to the equation

n=P V/ R T?

View answer and explanation

Correct option: B

It would be less than the actual value

It would be less than the actual value. The reaction is endothermic, so it absorbs heat from the surroundings (the reaction vessel). The temperature decreases, and since n = PV/RT, a lower temperature leads to a lower calculated value of n.

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The internal energy of one mole of a gas is: An ideal gas is allowed to expand both reversibly and irreversibly in an isolated system. If

{T_i}

is the initial temperature and

{T_f}

is the final temperature, which of the following statements is correct? For which of the process, ∆S is 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: 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. For the reaction,

\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1}

300 \mathrm{~K}

. Hence,

\Delta G