Answer:
Explanation:
The volume and amount are constant, so we can use Gay-Lussac’s Law:
At constant volume, the pressure exerted by a gas is directly proportional to its temperature.
Data:
p₁ = 1520 Torr; T₁ = 27 °C
p₂ = ?; T₂ = 150 °C
Calculations:
(a) Convert the temperatures to kelvins
T₁ = ( 27 + 273.15) K = 300.15 K
T₂ = (150 + 273.15) K = 423.15 K
(b) Calculate the new pressure
(c) Convert the pressure to atmospheres
<u>Answer:</u> The number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg
<u>Explanation:</u>
To calculate the amount of nitrogen gas, we use the equation given by ideal gas which follows:
where,
P = pressure of the gas = 755 mmHg
V = Volume of the gas = 2.55 L
T = Temperature of the gas =
R = Gas constant =
n = number of moles of nitrogen gas = ?
Putting values in above equation, we get:
To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law.
The equation follows:
where,
are the initial pressure, volume and temperature of the gas
are the final pressure, volume and temperature of the gas
We are given:
Putting values in above equation, we get:
Hence, the number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg