234k views
2 votes
A 7.50 liter sealed jar at 18 °c contains 0.125 moles of oxygen and 0.125 moles of nitrogen gas. what is the pressure in the container?

User Amnon
by
7.4k points

2 Answers

2 votes

Answer: The pressure of the container will be 0.796 atm.

Step-by-step explanation:

To calculate the mass of bromine gas, we use the ideal gas equation, which is:

PV = nRT

where,

P = pressure of the gas = ? atm

V = Volume of the gas = 7.5 L

n = Number of moles of gas = [0.125 + 0.125] = 0.25 mol

R = Gas constant =
0.0821\text{ L atm }mol^(-1)K^(-1)

T = temperature of the gas =
18^oC=(273+18)K=291K

Putting values in above equation, we get:


P* 7.5L=0.25mol* 0.0821\text{ L atm }mol^(-1)K^(-1)* 291K\\\\P=0.796atm

Hence, the pressure of the container will be 0.796 atm.

User Marquito
by
8.1k points
3 votes
The ideal gas equation is;
PV = nRT; therefore making P the subject we get;
P = nRT/V
The total number of moles is 0.125 + 0.125 = 0.250 moles
Temperature in kelvin = 273.15 + 18 = 291.15 K
PV = nRT
P = (0.250 × 0.0821 )× 291.15 K ÷ (7.50 L) = 0.796 atm
Thus, the pressure in the container will be 0.796 atm
User Apoq
by
8.7k points

No related questions found

Welcome to QAmmunity.org, where you can ask questions and receive answers from other members of our community.