(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

If 2.00 m³ of a gas initially at STP is placed under a pressure of 5.00 atm, the temperature of the gas rises to 39.0°C. What is the volume?

STP means it's at 0°C and 1 atm of Pressure, correct?

V1 = 2.00 m³

V2 = ?

T1 = 0°C = 273°K (My main confusion was units: °C vs. °K and atm vs. Pa)

T2 = 39°C = 312°K

P1 = 1 atm = 101.3 kPa

P2 = 6 atm = 607.8 kPa

R = 8.135

2. Relevant equations

P1*V1 = nR*T1 (nR is a constant) (I don't think I need to use this, but this one translates into the next equation)

(P1*V1)/(T1) = (P2*V2)/(T2)

3. The attempt at a solution

101.3*2/273 = 607.8*V2/312

.742 = 1.948*V2

V2 = .3809 m³

This makes sense to me, because pressure is inversely proportional to Volume. As pressure increases, Volume decreases. Am I correct in my work and thinking?

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# Homework Help: Thermodynamics Ideal Gas Law problem (pressure problem)

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