If 1.0 kcal of heat is added to 1.2 L of O 2 in a cylinder at constant pressure of 1 atm, the volume increases to 1.5 L. Calculate Δ H of the process (in kcal).

Question

If 1.0 kcal of heat is added to 1.2 L of O 2 in a cylinder at constant pressure of 1 atm, the volume increases to 1.5 L. Calculate Δ H of the process (in kcal). (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

w =- P text ext ( V 2- V 1)=-1(1.5-1.2)=-0.3 L atm =-7.235 cal Δ U = q + w =1-0.007235=0.993 kcal q =Δ H =1 kcal

Q. If $1.0 k c a l$ of heat is added to $1.2 L$ of $O_{2}$ in a cylinder at constant pressure of $1 a t m$ , the volume increases to $1.5 L$ . Calculate $Δ H$ of the process (in kcal).

$w = - P_{ext} (V_{2} - V_{1}) = - 1 (1.5 - 1.2) = - 0.3 L a t m = - 7.235 c a l$
$Δ U = q + w$
$= 1 - 0.007235 = 0.993 k c a l$
$q = Δ H = 1 k c a l$

Q. If 1.0kcal of heat is added to 1.2L of O2​ in a cylinder at constant pressure of 1atm, the volume increases to 1.5L. Calculate ΔH of the process (in kcal).

w=−Pext ​(V2​−V1​)=−1(1.5−1.2)=−0.3Latm=−7.235cal ΔU=q+w =1−0.007235=0.993kcal q=ΔH=1kcal

Q. If $1.0 k c a l$ of heat is added to $1.2 L$ of $O_{2}$ in a cylinder at constant pressure of $1 a t m$ , the volume increases to $1.5 L$ . Calculate $Δ H$ of the process (in kcal).

$w = - P_{ext} (V_{2} - V_{1}) = - 1 (1.5 - 1.2) = - 0.3 L a t m = - 7.235 c a l$
$Δ U = q + w$
$= 1 - 0.007235 = 0.993 k c a l$
$q = Δ H = 1 k c a l$