At constant temperature and pressure- which one of the following statement is correct for the reaction- CO g -1-2 O 2 g - CO 2 g A- - H - UB- - H - UC- - H - UD- - H is independent of the physical state of the reactants

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Enthalpy

At constant t...

Question

At constant temperature and pressure, which one of the following statement is correct for the reaction?
$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$

Δ H > Δ U

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Δ H < Δ U

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Δ H = Δ U

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Δ H

is independent of the physical state of the reactants

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Solution

The correct option is B $Δ H < Δ U$
We know, $Δ H = Δ U + P Δ V$ = $Δ U + n_{g} R T$
where $Δ H$ = Change in enthalpy
$Δ U$ = Change in internal energy
$n_{g}$ = $n_{p r o d u c t s} - n_{r e a c t a n t s}$
$n_{g}$ = $1 - 1.5$ = -0.5
So, $Δ U$ > $Δ H$

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Enthalpy

Standard XII Chemistry

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At constant temperature and pressure, which one of the following statement is correct for the reaction? CO(g)+12O2(g)→CO2(g)

The correct option is B ΔH<ΔUWe know, ΔH=ΔU+PΔV = ΔU+ngRT where ΔH = Change in enthalpy ΔU = Change in internal energy ng = nproducts−nreactants ng = 1−1.5 = -0.5 So, ΔU > ΔH

At constant temperature and pressure, which one of the following statement is correct for the reaction?
$C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g)$

The correct option is B $Δ H < Δ U$
We know, $Δ H = Δ U + P Δ V$ = $Δ U + n_{g} R T$
where $Δ H$ = Change in enthalpy
$Δ U$ = Change in internal energy
$n_{g}$ = $n_{p r o d u c t s} - n_{r e a c t a n t s}$
$n_{g}$ = $1 - 1.5$ = -0.5
So, $Δ U$ > $Δ H$