Question

What pressure is exerted by 852.9 g of CH₄ in a 0.910 L steel container at 137.2 K?

Answer 1

To calculate the pressure of CH4 in the container, first find the moles of gas using its molar mass, then use the ideal gas law with constants in the correct units for pressure.

Step-by-step explanation:

To determine the pressure exerted by 852.9 g of CH4 (methane) in a 0.910 L steel container at 137.2 K, we need to use the ideal gas law. The ideal gas law is PV = nRT, where P is pressure, V is volume, n is the number of moles of the gas, R is the ideal gas constant, and T is the temperature in Kelvin. First, we calculate the number of moles of CH4 using its molecular weight (16.04 g/mol) and then substitute into the ideal gas law using the appropriate value for R (which includes the units of pressure we want for our answer).

Here's a step-by-step solution:

1. Calculate moles of CH4: n = mass (in g) / molar mass (in g/mol) = 852.9 g / 16.04 g/mol
2. Calculate pressure: P = (nRT) / V

We would use 0.0821 (L*atm)/(mol*K) for R if we want the pressure in atmospheres.