0.5 mole each of two ideal gases A(Cv, m=(5/2) R) and B(Cv, m=3 R) are taken in a container and expanded reversibly and adiabatically, during this process temperature of gaseous mixture decreased from 350 K to 250 K. Find Δ H( in cal / mol ) for the process:

Question

0.5 mole each of two ideal gases A(Cv, m=(5/2) R) and B(Cv, m=3 R) are taken in a container and expanded reversibly and adiabatically, during this process temperature of gaseous mixture decreased from 350 K to 250 K. Find Δ H( in cal / mol ) for the process: (A) -100 R (B) -137.5 R (C) -375 R (D) None of these

Tardigrade Admin · Accepted Answer

text Δ H=(n1 Cp, m1+n2 Cp, m2) Δ T =(0.5 × (7/2) R +0.5 × 4 R )(-100) =-375 R ( Δ H is defined at cons. P )

Q. $0.5$ mole each of two ideal gases $A (C_{v, m} = \frac{5}{2} R)$ and $B (C_{v, m} = 3 R)$ are taken in a container and expanded reversibly and adiabatically, during this process temperature of gaseous mixture decreased from $350 K$ to $250 K$ . Find $Δ H ($ in $c a l / m o l$ ) for the process:

$- 100 R$

$- 137.5 R$

$- 375 R$

None of these

$Δ H = (n_{1} C_{p, m_{1}} + n_{2} C_{p, m_{2}}) Δ T$
$= (0.5 \times \frac{7}{2} R + 0.5 \times 4 R) (- 100)$
$= - 375 R$
( $Δ H$ is defined at cons. $P$ )

Q. 0.5 mole each of two ideal gases A(Cv,m​=25​R) and B(Cv,m​=3R) are taken in a container and expanded reversibly and adiabatically, during this process temperature of gaseous mixture decreased from 350K to 250K. Find ΔH( in cal/mol ) for the process:

−100R

−137.5R

−375R

None of these

ΔH=(n1​Cp,m1​​+n2​Cp,m2​​)ΔT =(0.5×27​R+0.5×4R)(−100) =−375R ( ΔH is defined at cons. P )

$- 100 R$

$- 137.5 R$

$- 375 R$

$Δ H = (n_{1} C_{p, m_{1}} + n_{2} C_{p, m_{2}}) Δ T$
$= (0.5 \times \frac{7}{2} R + 0.5 \times 4 R) (- 100)$
$= - 375 R$
( $Δ H$ is defined at cons. $P$ )