Respuesta :
Answer:
The answer to your question is below
Explanation:
1.-
Data
Pressure = ?
moles = 0.450
temperature = 25°C
Volume = 0.650 L
R = 0.082 atm L / mol °K
1) Convert temperature to °K
°K = 25 + 273
= 298°K
2) Use the Ideal gas law to solve this problem
PV = nRT
- Solve for P
P = nRT / V
- Substitution
P = (0.45)(0.082)(298) / 0.65
- Result
P = 16.91 atm
2.-
Pressure = 221 kPa
moles = 1
Volume = ?
Temperature = 32°C
R = 0.082 atm L /mol°K
Process
1) Convert pressure to atm
Pressure = 221 kPa = 221000 Pa
1 atm ----------------- 101325 Pa
x ------------------ 221000 Pa
x = (221000 x 1)/101325
x = 2.18 atm
2.- Convert temperature to °K
°K = 273 + 32 = 305°
3.- Substitution
PV = nRT
- Solve for V
V = nRT / P
- Substitution
V = (1)(0.082)(305) / 2.18
- Result
V = 11.47 L
Answer:
1) Pressure = 16.9 atm
2) The volume needed is 11.5 L
Explanation:
What pressure is exerted by 0.450 mol of a gas at 25°C if the gas is in a 0.650-L container?
p*V = n*R*T
⇒with p = the pressure = TO BE DETERMINED
⇒with V = the volume of the container = 0.650 L
⇒with n =the number of moles of gas = 0.450 moles
⇒ with R = the gas constant = 0.08206 L*atm /mol*K
⇒ with T = the temperature = 25 °C = 298 K
p = (n*R*T)/V
p = (0.450 * 0.08206 * 298) / 0.650
p = 16.9 atm
The recommended air pressure of a car tire is 32.0 psi (221 kPa). An average tire holds
around 1 mole of gas. What is the volume of the tire at 32°C?
p*V = n*R*T
⇒with p = the pressure = 32.0 psi = 221 kPa = 2.18 atm
⇒with V = the volume of the tire = TO BE DETERMINED
⇒with n =the number of moles of gas = 1.0 mol
⇒ with R = the gas constant = 0.08206 L*atm /mol*K
⇒ with T = the temperature = 32 °C = 305 K
V = (n*R*T) / p
V = 1.0 * 0.08206 * 305) / 2.18
V = 11.5 L
