Question

A 7.07 7.07 L cylinder contains 1.80 1.80 mol of gas A and 4.86 4.86 mol of gas B, at a temperature of 30.4 30.4 °C. Calculate the partial pressure of each gas in the cylinder. Assume ideal gas behavior.

Answer 1

The partial pressure of gas A is 6.34 atm

The partial pressure of gas B is 17.12 atm

Step-by-step explanation:

Step 1 :Data given

Volume of cylinder = 7.07 L

Number of moles gas A = 1.80 moles

Number of moles gas B = 4.86 moles

Temperature =30.4 ° C = 303.55 K

Step 2: Calculate pressure of gas A

p*V = n*R*T

p =(n*R*T)/V

⇒ with p = the partial pressure of gas A

⇒ with V = The volume of the cylinder = 7.07 L

⇒ with n = the number of moles gas A = 1.80 moles

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 303.55 K

p = (1.80 *0.08206 *303.55)/7.07

p = 6.34 atm

Step 3: Calculate pressure of gas B

p*V = n*R*T

p =(n*R*T)/V

⇒ with p = the partial pressure of gasB

⇒ with V = The volume of the cylinder = 7.07 L

⇒ with n = the number of moles gas B = 4.86 moles

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 303.55 K

p = (4.86 *0.08206 *303.55)/7.07

p = 17.12 atm

The partial pressure of gas A is 6.34 atm

The partial pressure of gas B is 17.12 atm

Answer 2

Answer: The partial pressure of gas A is 6.34 atm and that of gas B is 17.1 atm

Step-by-step explanation:

To calculate the pressure of the gas, we use the equation given by ideal gas, which follows:

`PV=nRT` ......(1)

where,

P = pressure of the gas

V = Volume of the gas

T = Temperature of the gas

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

n = number of moles of gas

• For Gas A:

We are given:

`V=7.07L\\T=30.4^oC=[30.4+273]K=303.4K\\n=1.80mol`

Putting values in equation 1, we get:

`p_A* 7.07L=1.80mol* 0.0821\text{ L atm }mol^(-1)K^(-1)* 303.4K\\\\p_(A)=(1.80* 0.0821* 303.4)/(7.07)=6.34atm`

• For Gas B:

We are given:

`V=7.07L\\T=30.4^oC=[30.4+273]K=303.4K\\n=4.86mol`

Putting values in equation 1, we get:

`p_B* 7.07L=4.86mol* 0.0821\text{ L atm }mol^(-1)K^(-1)* 303.4K\\\\p_(B)=(4.86* 0.0821* 303.4)/(7.07)=17.1atm`

Hence, the partial pressure of gas A is 6.34 atm and that of gas B is 17.1 atm