Solve
Guides
0
You visited us 0 times! Enjoying our articles? Unlock Full Access!
Standard XI
Chemistry
Applications of First Law of Thermodynamics
Question

As a 1.00-mol sample of a monatomic ideal gas expands adiabatically, the work done on it is $$-2.50 \times 10^3 J$$. The initial temperature and pressure of the gas are 500 K and 3.60 atm. Calculate (a) the final temperature and(b) the final pressure.

Open in App
Solution
Verified by Toppr


Was this answer helpful?
1
Similar Questions
Q1
The work done in adiabatic compression of 2 moles of an ideal monatomic gas by the constant external pressure of 2 atm starting from an initial pressure of 1 atm and an initial temperature of 300 K is:
[R = 2 cal/mol-K]

View Solution
Q2
One mole of an ideal gas ⟮Cv,m=52R⟯ at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is:
View Solution
Q3
One mole of a monoatomic ideal gas expands adiabatically at initial temperature T against a constant external pressure of 1atm from 1 litre to 3 litres. The final temperature of the gas is
View Solution
Q4
An ideal monoatomic gas (Cv=1.5 R) initially at 298 K and 1.013 atm expands adiabatically irreversibly until it is in equilibrium with a constant external pressure of 0.1013 atm. The final temperature (in Kelvin) of the gas is :
View Solution
Q5
One mole of an ideal gas [Cv,m=52R] at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. The final temperature (in Kelvin) of the gas is:
View Solution