NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

1 of 1

Application +4 | -1

x

g sample of

\mathrm{NH}_4 \mathrm{NO}_3

is decomposed in a Bomb calorimeter. The temperature of calorimeter increase by

4^{\circ} \mathrm{C}

. The heat capacity of the system is

125 \mathrm{~kJ} /{ }^{\circ} \mathrm{C}

. The value of

x

is
(Given molar heat of decomposition of

\mathrm{NH}_4 \mathrm{NO}_3

at constant volume is

400 \mathrm{~kJ} \mathrm{~mol}^{-1}

)

View answer and explanation

Correct option: A

Option A (1) is correct because it represents the mass of NH4NO3 required to produce the given temperature change in the calorimeter, calculated using the heat capacity and molar heat of decomposition.

More Questions from THERMODYNAMICS

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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