Here is the full question
A 2.37 L balloon contains .115 mol of xenon gas, Xe(g), at a pressure of 954 Torr. What is the temperature, in Kelvin, of the Xe in the balloon? Express the answer using 3 significant figures.
Answer:
Temperature of Xenon = 313.77 K
Explanation:
Given that: volume of the balloon v = 2.37 L
number of mole n = 0.115 mol
gas constant R = 0.0821 L.atm/mol.K
temperature T = ? (in Kelvin)
pressure P = 954 torr (in atm)
since;
1 atm ----------- 760 torr
y atm ----------- 954 torr
760 y = 954
y = 954/760
y ≅ 1.25
Pressure P = 1.25 atm
Using ideal gas equation (gas equation); we have the following expression:
[tex]P*V = n*R*T[/tex]
Making T the subject of the formula; we have:
[tex]T = \frac{PV}{nR}[/tex]
[tex]T = \frac{1.25 * 2.37}{0.115 *0.0821}[/tex]
T = 313.77 K
Thus; the Temperature of Xenon = 313.77 K
Answer:
The temperature in the balloon is 315 K
Explanation:
The full question
A 2.37 L balloon contains 0.115 mol of xenon gas, Xe(g), at a pressure of 954 Torr. What is the temperature, in Kelvin, of the Xe in the balloon?
Step 1: Data given
Volume of the balloon = 2.37 L
Number of moles Xenon gas = 0.115 moles
Pressure of the gas = 954 torr = 954 / 760 atm = 1.25526 atm
Step 2: Calculate the temperature of the xenon gas
p*V = n*R*T
⇒with p = the pressure of wenon gas = 1.25526 atm
⇒with V = the volume of the balloon = 2.37 L
⇒with n = the number of moles of xenon = 0.115 moles
⇒with R = the gasconstant = 0.08206 L*atm/mol*K
⇒with T = the temperature in the balloon = TO BE DETERMINED
T = (p*V) / (n*R)
T = (1.25526 * 2.37)/(0.115 * 0.08206)
T = 315 K
The temperature in the balloon is 315 K
