# UNIT 7: Thermodynamics - Online Test

Q1. The amount of heat exchanged with the surrounding at constant temperature and pressure is given by the quantity
Explaination / Solution:
No Explaination.

Q2. All the naturally occurring processes proceed spontaneously in a direction which leads to
Explaination / Solution:
No Explaination.

Q3. In an adiabatic process, which of the following is true ?
Explaination / Solution:
No Explaination.

Q4. In a reversible process, the change in entropy of the universe is
Explaination / Solution:
No Explaination.

Q5. In an adiabatic expansion of an ideal gas
Explaination / Solution:
No Explaination.

Q6. The intensive property among the quantities below is
Explaination / Solution:
No Explaination.

Q7. An ideal gas expands from the volume of 1 × 10–3 m3 to 1 × 10–2 m3 at 300 K against a constant pressure at 1 × 105 Nm–2. The work done is
Explaination / Solution:

w = – P V

w = – (1 × 105 Nm–2)

(1× 10–2 m3 – 1 × 10–3 m3)

w= –105 (10–2 – 10–3) Nm

w = – 105 (10 – 1) 10–3) J

w = – 105 (9 × 10–3) J

w = –9 × 102 J w = –900 J

Q8. Heat of combustion is always
Explaination / Solution:
No Explaination.

Q9. The heat of formation of CO and CO2 are – 26.4 kCal and – 94 kCal, respectively. Heat of combus-tion of carbon monoxide will be
Explaination / Solution:

CO (g )+1/2O2 (g )→CO 2 (g)

ΔHC0 (CO) = ΔHf (CO2) – ΔHf(CO) + ΔHf (O2)]

ΔHC0 (CO) = ΔHf (CO2) – ΔHf(CO) + ΔHf (O2)]

ΔHC0 (CO) = – 94 KCal – [– 26.4 KCal + 0]

ΔHC0 (CO) = – 94 KCal + 26.4

KCal ΔHC0 (CO) = – 67.4 Kcal

Q10. C(diamond) → C(graphite), ∆H = –ve, this indicates that
Explaination / Solution:
No Explaination.