${\rm{C}} + {{\rm{O}}_2} \to {\rm{C}}{{\rm{O}}_2};$ ${\rm{CO}} + \frac{1}{2}{{\rm{O}}_2} \to {\rm{C}}{{\rm{O}}_2}$ Then the heat of formation of CO is

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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\mathrm{C} + {\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2};

\mathrm{CO} + \frac{1}{2}{\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2}

Then the heat of formation of CO is

View answer and explanation

Correct option: A

X-Y

Option A (X-Y) is correct because the heat of formation of CO can be found by subtracting the heat of the second reaction from the heat of the first reaction based on Hess's Law.

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