Calculate the change in entropy when two gram atoms of aluminium is heated from 25°C to 600°C. The atomic heat capacity of aluminium is given by Cp = 5.006 + 0.0026 T cal/deg.

Question

Calculate the change in entropy when two gram atoms of aluminium is heated from 25°C to 600°C. The atomic heat capacity of aluminium is given by Cp = 5.006 + 0.0026 T cal/deg. (A) 23.75 cal/deg (B) 6.8 eu (C) 13.75 eu (D) 10 eu

Tardigrade Admin · Accepted Answer

The process takes place at constant pressure. Hence,

Δ Q = C_{p} Δ T

and

Δ S = \int_{T_{1}}^{T_{2}} \frac{n C _{p} d T}{T} = 2 \int_{298}^{873} (\frac{5.006}{T} + 0.0026) d T

= 2 [5.006 l n \frac{873}{298} + 0.0026 (873 - 298)]

= 2 [5.381 + 1.495] = 13.75 c a l / d e g

or

13.75 e u

Q. Calculate the change in entropy when two gram atoms of aluminium is heated from $2 5^{°} C$ to $60 0^{°} C$ . The atomic heat capacity of aluminium is given by $C_{p} = 5.006 + 0.0026 T c a l / d e g$ .

$23.75 c a l / d e g$

$6.8 e u$

$13.75 e u$

$10 e u$

The process takes place at constant pressure. Hence, $Δ Q = C_{p} Δ T$
and $Δ S = \int_{T_{1}}^{T_{2}} \frac{n C _{p} d T}{T} = 2 \int_{298}^{873} (\frac{5.006}{T} + 0.0026) d T$
$= 2 [5.006 l n \frac{873}{298} + 0.0026 (873 - 298)]$
$= 2 [5.381 + 1.495] = 13.75 c a l / d e g$ or $13.75 e u$

Q. Calculate the change in entropy when two gram atoms of aluminium is heated from 25°C to 600°C. The atomic heat capacity of aluminium is given by Cp​=5.006+0.0026Tcal/deg.

23.75cal/deg

6.8eu

13.75eu

10eu