Question

45.6 grams of CH4 is placed into a 275 mL container at 55.00C. What is the pressure inside the container in atm?

Answer 1

Given-

Mass of CH4 - 45.6 grams

Molar mass of CH4 - 16.04 g/mol

volume - 275mL

Temperature- 55°C

Solution,

moles of methane (CH4) n = 45.6/16.04

= 2.84 moles

Using Formula,

Pv = nRT

P*275 = 2.84*8.314*55

P = 1298.64/275

P = 4.72 Atm.

Answer - The pressure inside the container in atm is 4.72.

Answer 2

45.6 grams of CH4 is placed into a 275 mL container at 55.00 C. The pressure is 4.72 atm.

What is partial pressure?

The pressure that one of the gases in a mixture would exert if it were in the same volume on its own.

Given the mass is 45.6 grams

The volume is 275 L

Temperature is 55.00 C.

Calculate the moles

$\rm Number\;of \;moles= \dfrac{mass}{molar\;mass}\\\\\rm Number\;of \;moles= \dfrac{45.6}{16.04} = 2.84 moles$

Now, calculating the pressure

PV = nRT

$P\times 275 = 2.84\times 8.314\times 55 = 4.72 atm.$

Thus, the pressure inside the container in is 4.72 atm.

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