Heat energy change during the chemical reaction, ${\rm{CO}} + \frac{1}{2}{{\rm{O}}_2} \to {\rm{C}}{{\rm{O}}_2}$is known as :

Latent heat of ${\rm{C}}{{\rm{O}}_2}$

Heat of formation of ${\rm{C}}{{\rm{O}}_2}$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Heat energy change during the chemical reaction,

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

is known as :

View answer and explanation

Correct option: A

Heat of combustion of CO

Option A (Heat of combustion of CO) is correct because the reaction describes the complete burning of CO in oxygen to form CO2, which is the definition of heat of combustion.

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