What pressure is exerted by 974.7 g of CH4 in a 0.570 L steel container at 199.3 K ?

Answer 1

You need to know Ideal gas formula PV=nRT , P is the pressure in atm which at our atmospheric pressure is P_atm =1 atm , V is the volume of container , n- number of moles, R is the gas constant 0.082 atm.L.mol^-1k^-1.

Now that you know the formula you need to do unit conversions and plug them in this equation.

1. first find the number of moles of CH₄ by using molar mass 974.7 g CH₄× 1 mole CH₄ ⁄ 16 g CH₄ = 60.92 moles of CH4
2. Pv=nRT P=nRT/V P=(60.92 mole ×0.082atm.L.mol^-1k^-1.× 199.3 K) ⁄ 0.570 L
3. plug this in your calculator and you will find your pressure in atm. for practice think about what it would be in mmHg instead of atm

Answer 2

Use the IGL P = nRT/V You will need moles of CH₄. T and V are in the proper units for R = .0820574 for P in atm. .0831446 for P in bars). Your answer should keep 4 sig figs, so you need your gas constant to have more of them.

n = m/M or 974.7 g CH₄ * (1 mole/16.04 g CH₄) The molar masses are actually limited to 4 sig figs as they are averages and change with circumstances.

I'll leave the rest to you. Please consider a tutor. Take care.