Question

9. What is the molar volume of a gas if the atmospheric pressure and the temperature are 700 mmHg and 50°F? Show your work. (5 points)

Answer 1

700 mm Hg = 0.933257 bar I 50°F U = 283.15 K il 1 mmHg = 0.0013322 bar) i [l'F = 255.928 k] - use equation PV = nRT where = volume in litre... n = males / number of moles. P = Pressure of gas. R = gos constant value T = temperature at 273.15 K = 8-3 14 x 10 bart molk

So, So, given are pressure = 700 mm Hg ar =0.933 257 bar Temperature = 283 · 15k PV = nRT V = nRT - P V = 1 mol X 8.314 X 102 bar XL X 283.15 K - molk 0.933 257 bar

Valume v = 25:22 4 6 Litre ar v= 25.22 L