Physics question here help please.Is my solution correct?

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In summary, a gas with 4 moles, initially at 300 K and 10 atm, undergoes a change of state with a decrease in temperature of 50 K and an increase in volume of 10 liters. To find the final temperature and volume, we can use the equation P*v=n*R*T and the given information to find V1 and then use V2=V1+∆V to find the final volume. However, when doing this calculation, one should pay attention to units and use the correct value for pressure (10 atm instead of just 10).
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A moster of a gas has 4 moles and first is in the temperature 300 K and pressure 10 atmosphere.After a change of state, ∆T= -50 K and ∆V=10 liter.Find the final temperature ,volume and pressure of the gas.


2. Homework Equations

P*v=n*R*T

3. The Attempt at a Solution
So T2-T1=-50 <=> T2=300-50=250 K
Now,to find V2, I thought : Find V1 first and then do V2-V1=∆V. From pv=nRT where T =300,pressure is 10 and the moles are 4. I Find that V1=997.2 here I replace V2-997.2=10 but V2 isn't the same as in my textbook..what did I do wrong
 
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  • #2
Try to work with units, this could help. I don't think V1=997.2 liters, and if it is something else you cannot simply add 10 to the numerical value.
 
  • #3
Take a look again at your pressure... It is 10 atmospheres not just 10. You will end up with a much smaller value for volume
 

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