Respuesta :
a) Under constant pressure conditions, volume is directly proportional to the temperature. i.e,
V α T
V1/T1 = V2/T2 -----(1)
It is given that: V2 = 1/3 V1
Substituting for V2 in equation (1) gives:
1/T1 = 1/3T2
i.e. T2 = (1/3) T1
2) Based on the ideal gas equation:
PV = nRT
Under constant n and R
P1V1/T1 = P2V2/T2
P2 = (P1V1/T1)*T2/V2 = (4*5.5/300)*250/2 = 9.17 atm
3) As per Raoult's Law, partial pressure of a gas is equal to the product of mole fraction and the total gas pressure
Mole fraction of Ne = 0.50/0.50 + 1.20 = 0.294
Total pressure = 730 torr
Partial Pressure of Ne = 0.294*730 = 215 torr
Answer:
If you decreased the volume of a sample of gas by a factor of three while maintaining a constant pressure, how would the absolute temperature of the gas be affected?
✔ it would decrease threefold
A gas at 300 K and 4.0 atm is moved to a new location with a temperature of 250 K. The volume changes from 5.5 L to 2.0 L. What is the pressure of the gas at the new location?
✔ 9.2 atm
What is the partial pressure of 0.50 mol Ne gas combined with 1.20 mol Kr gas at a final pressure of 730 torr?
✔ 215 torr
Explanation:
there you go boo YW :)
