Question

At what Celsius temperature does 10.5 g of methane gas (CH4) under a pressure of 1.77 atm occupy 35.6 L? Assume the methane is ideal.

Answer 1

Answer: 889.73 Celsius

Step-by-step explanation:

ideal gas law

pv=nRT

P= 1.77 atm

v=35.6 L

R=.0821 L.atm/mol.k

n = moles so you must take the 10.5 g methane(CH4) and convert to moles

10.5 /16 = 0.66 moles

T answer will be in Kelvin so after calculating you will subtract 273.15 to get it in celsius

T= PV/nR = 1.77 x35.6 /(0.66 X 0.0821)=1162.88 K -273.15 = 889.73 celsius