Respuesta :
Answer: The partial pressure of gas A is 6.34 atm and that of gas B is 17.1 atm
Explanation:
To calculate the pressure of the gas, we use the equation given by ideal gas, which follows:
[tex]PV=nRT[/tex] ......(1)
where,
P = pressure of the gas
V = Volume of the gas
T = Temperature of the gas
R = Gas constant = [tex]0.0821\text{ L. atm }mol^{-1}K^{-1}[/tex]
n = number of moles of gas
- For Gas A:
We are given:
[tex]V=7.07L\\T=30.4^oC=[30.4+273]K=303.4K\\n=1.80mol[/tex]
Putting values in equation 1, we get:
[tex]p_A\times 7.07L=1.80mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 303.4K\\\\p_{A}=\frac{1.80\times 0.0821\times 303.4}{7.07}=6.34atm[/tex]
- For Gas B:
We are given:
[tex]V=7.07L\\T=30.4^oC=[30.4+273]K=303.4K\\n=4.86mol[/tex]
Putting values in equation 1, we get:
[tex]p_B\times 7.07L=4.86mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 303.4K\\\\p_{B}=\frac{4.86\times 0.0821\times 303.4}{7.07}=17.1atm[/tex]
Hence, the partial pressure of gas A is 6.34 atm and that of gas B is 17.1 atm
Answer:
The partial pressure of gas A is 6.34 atm
The partial pressure of gas B is 17.12 atm
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
