Question

The pressure in a 5.75 L container of 48.0 g of bromine gas at 100.0°C is

Answer 1

Assuming the gas is ideal, we can use the Ideal Gas Law:
PV = nRT
where
P = pressure in atm
V = volum in liters
n = number of moles
R = universal gas constant = 0.0821 L-atm/mol-K
T = temperature in Kelvin
We know V, T and of course, R. To convert degree Celsius to Kelvin, we just add 273. To get n, we divide the given mass by the molar mass of bromine. The mass of Br is 79.9, but since it is diatomic (Br2) the molar mass is 79.9 x 2 = 159.8 g/mol
Thus,
n = 48 / 159.8 = 0.300375 mol Br2
Substituting,
PV = nRT
P = nRT / V
P = (0.300375)(0.0821)(100 + 273) / 5.75

Now solve for P. Units are in atm.
Hope this helps :3

Answer 2

1.6