Question

if 4.5g of methane gas CH to the fourth is in a 2.0L container at 35 degree Celsius. What is the pressure of the container?

Answer 1

The pressure of the container is approximately 3.63 atm.

Step-by-step explanation:

To find the pressure of the container, we can use the Ideal Gas Law, which is expressed as PV = nRT, where P is the pressure, V is the volume, n is the number of moles of the gas, R is the gas constant, and T is the temperature in Kelvin.

In this case, we are given the volume (2.0 L) and the temperature (35 °C = 308 K).

First, we need to convert the temperature to Kelvin by adding 273 to Celsius. So, T = 35 + 273 = 308 K.

We are also given the mass of the methane gas (4.5 g), but we need to convert it to moles. The molar mass of methane (CH4) is 16 g/mol. So, the number of moles of methane is given by moles = mass / molar mass = 4.5 g / 16 g/mol = 0.28125 mol.

Now we can plug the values into the Ideal Gas Law equation to solve for the pressure:

PV = nRT

P * 2.0 L = 0.28125 mol * 0.0821 L.atm/mol.K * 308 K

P * 2.0 L = 7.2633 L.atm

P = 7.2633 L.atm / 2.0 L = 3.63165 atm

Therefore, the pressure of the container is approximately 3.63 atm.