Physics question here help please.Is my solution correct?

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The discussion revolves around solving a gas law problem involving a gas with 4 moles at an initial temperature of 300 K and pressure of 10 atmospheres, which undergoes a change in state with a temperature decrease of 50 K and a volume increase of 10 liters. The initial attempt to calculate the final temperature, volume, and pressure is presented, but the user questions the accuracy of their volume calculation. Feedback suggests that the initial volume calculation may be incorrect due to misinterpretation of the pressure unit, emphasizing the importance of unit consistency. The user is advised to re-evaluate their calculations, particularly focusing on the pressure being 10 atmospheres rather than a simple numerical value. Correcting these errors is crucial for obtaining the accurate final state of the gas.
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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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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.
 
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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