Can someone please explain this chemistry question to me part a and part b please write neatly
a)You have a gaseous nitrogen (N2) system at a fixed temperature and pressure. If 25 grams occupies 0.125 liters, how much volume would 14 moles occupy?
b) You have a gaseous system with the following properties. Pressure = 725 mmHg Temperature = 27 °C Volume = 7.5 mL How many moles of gaseous particle do you have
a)
Molar mass of N2 = 28.02 g/mol
mass of N2 = 25 g
we have below equation to be used:
number of mol of N2,
n = mass of N2/molar mass of N2
=(25.0 g)/(28.02 g/mol)
= 0.8922 mol
we have:
V1 = 0.125 L
n1 = 0.8922 mol
n2 = 14 mol
we have below equation to be used:
V1/n1 = V2/n2
0.125 L / 0.8922 mol = V2 / 14 mol
V2 = 1.96 L
Answer: 1.96 L
b)
we have:
P = 725.0 mm Hg
= (725.0/760) atm
= 0.9539 atm
V = 7.5 mL
= (7.5/1000) L
= 0.0075 L
T = 27.0 oC
= (27.0+273) K
= 300 K
find number of moles using:
P * V = n*R*T
0.9539 atm * 0.0075 L = n * 0.0821 atm.L/mol.K * 300 K
n = 2.9*10^-4 mol
Answer: 2.9*10^-4 mol
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