Respuesta :
Answer: The number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg
Explanation:
To calculate the amount of nitrogen gas, we use the equation given by ideal gas which follows:
[tex]PV=nRT[/tex]
where,
P = pressure of the gas = 755 mmHg
V = Volume of the gas = 2.55 L
T = Temperature of the gas = [tex]23^oC=[23+273]K=296K[/tex]
R = Gas constant = [tex]62.364\text{ L.mmHg }mol^{-1}K^{-1}[/tex]
n = number of moles of nitrogen gas = ?
Putting values in above equation, we get:
[tex]755mmHg\times 2.55L=n\times 62.364\text{ L.mmHg }mol^{-1}K^{-1}\times 296K\\\\n=\frac{755\times 2.55}{62.364\times 296}=0.1043mol[/tex]
To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law.
The equation follows:
[tex]\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}[/tex]
where,
[tex]P_1,V_1\text{ and }T_1[/tex] are the initial pressure, volume and temperature of the gas
[tex]P_2,V_2\text{ and }T_2[/tex] are the final pressure, volume and temperature of the gas
We are given:
[tex]P_1=755mmHg\\V_1=2.55mL\\T_1=23^oC=[23+273]K=296K\\P_2=?\\V_2=4.10L\\T_2=18^oC=[18+273]K=291K[/tex]
Putting values in above equation, we get:
[tex]\frac{755mmHg\times 2.55L}{296K}=\frac{P_2\times 4.10L}{291K}\\\\P_2=\frac{755\times 2.55\times 291}{4.10\times 296}=461.6mmHg[/tex]
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
Answer:
The final pressure is 461.6 mm Hg
Explanation:
Step 1:Data given
Volume of N2 = 2.55L
Pressure N2 = 755 mm Hg
Temperature = 23.0 °C
New volume = 4.10 L
Temperature = 18.0 °C
Step 2: Calculate the fina pressure
P1V1/T1 = P2V2/T2
P2 = P1V1/T1 * T2/V2
⇒ with P1 = initial pressure = 755/760 atm =0.993421 atm
⇒ with V1 = the initial volume = 2.55L
⇒ with T1 = the initial temperature = 23.0 °C = 296 K
⇒ with P2 = The final pressure
⇒with V2 = the new volume = 4.10 L
⇒with T2 = the new temperature = 18.0 °C = 291 K
P2 = 755 mm *2.55 L *296K/(291 K* 4.10 L) = 461.6 mm Hg
The final pressure is 461.6 mm Hg
