[Exit Strategy v1]

Wow. I am totally stumped. I am taking an at home Chemistry class just to improve my understanding of the subject better for next year at college and I came to this one question that seems easy but then it is so confusing.

What is the pressure of a gas if 300mL at 0.8 atm and 37 degrees C changes to 50 degrees C and 555mL?

Stumped totally. Any help on this one would be deeply appreciated.

[Linkiroth]

Combined Gas Law:

(P₁ V₁)/T₁ = (P₂ V₂)/T₂

Plug in the numbers and figure it out.

[Exit Strategy v1]

whoops. I just put the values in the wrong way. thank you for correcting that formula for me.

what i got was:
0.8atm x 300mL/37 Degrees C = P1 555mL/50 Degrees C and got .58atm

Did I hit it?

[sdekivit]

no, because you didn't use the absolute temperature in K. When you convert degrees C to kelvin and plug that number in, you'll get the correct answer.

[camur]

Remember the ideal gas equation PV=nRT  temperature scale must be in Kelvine. The number of moles and R are  constant.So PV/T will be constant.  
(0.8x300)/310=(P'x555)/323
then solve the equation for P'

[sdekivit]

remember that in this case we have to plug in the temperature. This means the absolute temperature in K. In another formula, Q = c * m * delta T, we have to plug in a change in temperature and then we can plug in Celsius, since the change in Celsius equals the change in Kelvins.