A 500 mL metal cylinder holding 0.100 moles of helium gas is known to rupture at a pressure of 10 atmospheres. At what temperature, in °C, will the container fail?

Question

Here is what I came up with:

T= (1.00mol x 0.0821 LxATM/KxMOL) / 10atm x 0.5L

=0.01642K

Convert to C: 0.01642K - 273 = -272.98 C

That can't possibly be right. Please help.

Answer 1

No that is correct the answer will turn out to be a negative number.

Answer 2

I was giving the answer key with the correct answer at 336 C.

Now i'm really confused... Can someone explain.

Answer 3

Note that you substituted 1.00 mole for n and not 0.100 mol; also, you inverted the formula when you solved for T.
PV = nRT and rearrange to
T = PV/nR = (10)(0.500)/(0.100)(0.08206) = 609.3 K
609.3-273.15 = 336.16 which rounds to 336 C.

Answer 4

I recalculated the problem and got it correct. Thank you.

Answer 5

stupid responder