part a) If 41.2 L of N 2 at 32.8°C and 735 torr is heated to 119°C and compresse

Question

part a) If 41.2 L of N2 at 32.8°C and 735 torr is heated to 119°C and compressed to 2.91 L, what is the new pressure in torr? Enter your answer in scientific notation.

_____ × 10 ______torr

part b) At 85.0°C and 798 torr, calculate the number of moles and mass of 4.66 L of CH4 gas.

____mol

_____g

part a) If 41.2 L of N2 at 32.8°C and 735 torr is heated to 119°C and compressed to 2.91 L, what is the new pressure in torr? Enter your answer in scientific notation.

_____ × 10 ______torr

part b) At 85.0°C and 798 torr, calculate the number of moles and mass of 4.66 L of CH4 gas.

____mol

_____g

Explanation / Answer

Part A

PV= nRT

P = 735 torr or 0.967 atm

V = 41.2 L

n= ?

R = gas constant 0.0821 L atm K-1 Mol-1

T = 273 +38 = 311.

Substitute in the equation

0.967 x 41.2 = n x 0.0821 x 311

n = 1.56 Mole

Pressure at 119 °C and Volume 2.91 L

T = 273 +119 = 392

V = 2.91 L  

n = 1.56 Mole

P x 2.91 = 1.56 x 0.0821 x 392

P = 17.25 atm or 1.311 x 104 Torr

Part B

PV = nRT

P = 798 torr or 1.05 atm

V = 4.66

R = Gas constant 0.0821 L atm K-1 Mol-1

T = 273 +85 = 358

Substitute in the equation

1.05 x 4.66 = n x 0.0821 x 358

n = 0.16647 Mole CH4 gas present

Weight of CH4 gas = 0.16647 x 16 = 2.66 gm

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