Question

Calculate the volume of 53.0 g of (CH4) methane gas at 40°C and 2.0 atm. (C – 12.00 g/mol, H – 1.007 g/mol)

Answer 1

Explanation:

A variation of the Ideal Gas Equation: TRnVP. = mole ... methane at 25°C and 745 torr? ... mol. CHg mol g n. 8.40. 04.16. 1. 655. 4. = ×. = TK = 25°C + 273 = 298 K.

Answer 2

Answer: The volume of the gas is 4309.3ml.

Given: Pressure =2atm , Given mass of methane = 53g, Temperature =40°C+273= 313K.

To find: Volume of the gas.

Explaination: First we calculate the no. Of moles of methane gas,

No. Of moles =Given mass/molar mass

=53/16 (molar mass of methane=16g)

= 3.312moles.

Now we calculate, Volume of the gas by ideal gas formula,

PV=nRT

2×V = 3.312× 8.314×313

V= 4309.3ml.

Ideal gas law

• The general gas equation, commonly referred to as the ideal gas law, represents the state of a ideal gas through an equation, PV=nRT.
• According to the ideal gas law, the sum of the absolute temperature of the gas and the universal gas constant is equal to the product of the pressure and volume of one gram of an ideal gas.

To learn more about ideal gas, refer these links.

https://brainly.in/question/7432529

https://brainly.in/question/6239862

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