At constant T and p which one of the following statements is correct for the reaction? CO ( g )+(1/2) O 2( g ) longrightarrow CO 2( g )

Question

At constant T and p which one of the following statements is correct for the reaction? CO ( g )+(1/2) O 2( g ) longrightarrow CO 2( g ) (A)  Δ H>Δ E  (B)  Δ H<Δ E  (C)  Δ H=Δ E  (D)  Δ H is independent of physical state of reactants

Tardigrade Admin · Accepted Answer

Key Idea The relation between Δ H and Δ E is given by Δ H=Δ E+Δ ng R T where Δ ng= Sigma product of gaseous mole - Sigma reactant of gaseous mole For the reaction CO (g)+(1/2) O 2(g) longrightarrow CO 2(g) Δ ng=(1 mol. of .CO 2) - (1 mol. of CO +0.5 mol of O 2 ) Δ ng=-0.5, ie, it is negative. Hence, Δ H < Δ E If Δ ng=0, Δ H =Δ E Δ ng =+ text ve Δ H > Δ E

Q. At constant $T$ and $p$ which one of the following statements is correct for the reaction?
$CO (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)$

$Δ H > Δ E$

$Δ H < Δ E$

$Δ H = Δ E$

$Δ H$ is independent of physical state of reactants

Q. At constant T and p which one of the following statements is correct for the reaction? CO(g)+21​O2​(g)⟶CO2​(g)

ΔH>ΔE

ΔH<ΔE

ΔH=ΔE

ΔH is independent of physical state of reactants

Q. At constant $T$ and $p$ which one of the following statements is correct for the reaction?
$CO (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)$

$Δ H > Δ E$

$Δ H < Δ E$

$Δ H = Δ E$

$Δ H$ is independent of physical state of reactants