Chemistry College

A 7.95 L
container holds a mixture of two gases at 25 °C.
The partial pressures of gas A and gas B, respectively, are 0.352 atm
and 0.715 atm.
If 0.240 mol
of a third gas is added with no change in volume or temperature, what will the total pressure become?

Answers

Answer 1
To solve this problem, we can use the ideal gas law equation:

PV = nRT

where:
P = pressure
V = volume = 7.95 L
n = number of moles
R = gas constant = 0.08206 L atm K^-1 mol^-1
T = temperature = 25°C = 298 K

We can start by calculating the total number of moles of gas in the container before the third gas is added:

n_total = (P_A + P_B) V/RT

n_total = [(0.352 atm) + (0.715 atm)](7.95 L)/(0.08206 L atm K^-1 mol^-1)(298 K)

n_total = 6.06 mol

We know that 0.240 mol of a third gas is added, so the total number of moles of gas becomes:

n_total = 6.06 mol + 0.240 mol

n_total = 6.30 mol

Now we can use the ideal gas law to calculate the total pressure of the mixture:

P_total = n_total RT/V

P_total = (6.30 mol)(0.08206 L atm K^-1 mol^-1)(298 K)/(7.95 L)

P_total = 0.239 atm

Therefore, the total pressure of the mixture after the third gas is added is 0.239 atm.

:)’

Related Questions

If an aqueous solution is 5.321m, which of the following statements is incorrect?
A) Freezing point of solution will lower by 10 C
B) Boiling point of solution will increase by 2.72 C
C) Boiling point of solution will be 100 C
D) Osmotic pressure of solution will be higher than water

Answers

Boiling point of solution will be 100 C. The incorrect statement is C)

What is aqueous solution ?

An aqueous solution is one in which water serves as the solvent. One or more substances are dissolved in water to create such a solution, and the water molecules surround and separate the individual solute particles to create a homogeneous mixture.

Therefore, A solvent's boiling point and freezing point change when a solute is dissolved in it, respectively. Boiling point elevation and freezing point depression are two terms used to describe this occurrence. The concentration of the solute determines how much of an impact it has.

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A 1.5 M solution of HCl has 145 g of HCl dissolved, what is the volume of the solution?

Answers

The volume of the 1.5M solution of HCl solution that has 145g of mass is 2.65L.

How to calculate volume?

The volume of a solution can be calculated by dividing the number of moles by its molar concentration as follows;

Volume = no of moles ÷ molarity

According to this question, a 1.5M solution of HCl has 145g of mass. The number of moles can be calculated as follows:

no of moles = 145g ÷ 36.5g/mol = 3.973 moles

volume of HCl solution = 3.973mol ÷ 1.5M

volume of HCl = 2.65L

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