Question

($\Delta H - \Delta U$) for the formation of carbon monoxide (CO) from its elements at 298 K is (R = 8.314 J K⁻¹ mol⁻¹)(a) –2477.57 J mol⁻¹ (b) 2477.57 J mol⁻¹(c) –1238.78 J mol⁻¹ (d) 1238.78 J mol⁻¹

Answer 1

$\Delta H-\Delta U$ for the formation of carbon monoxide (CO) from its elements at 298 K is 1238.78J/mol

Explanation:

The standard enthalpy of formation or standard heat of formation of a compound is the change of enthalpy during the formation of 1 mole of the substance from its constituent elements, with all substances in their standard states.

The formation of carbon monoxide (CO) from its elements is represented as:

$C(s)+\frac{1}{2}O_2(g)\rightarrow CO(g)$

$\Delta H=\Delta U+\Delta n_g\times RT$

where,

$\Delta H$ =  enthalpy of the reaction

$\Delta U$= internal energy of the reaction

$\Delta n_g$ = change in the moles of the reaction = Moles of product - Moles of reactant = 1 - 0.5 = 0.5 mole

R = gas constant = 8.314 J/mole.K

T = temperature = 298 K

Putting in the values we get:

$\Delta H-\Delta U=0.5\times 8.314\times 298$

$\Delta H-\Delta U=1238.78J/mol$

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