Q1) One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1
ID: 880505 • Letter: Q
Question
Q1)
One mole of an ideal gas is sealed in a 22.4-L container at a pressure of 1 atm and a temperature of 273 K. The temperature is then increased to 304 K , but the container does not expand. What will the new pressure be?
Part A
The most appropriate formula for solving this problem includes only which variables?
Enter the required variables, separated by commas (e.g., P,V,T).
Q2)A sample of nitrogen gas in a 1.69-L container exerts a pressure of 1.37 atm at 17 C.
-What is the pressure if the volume of the container is maintained constant and the temperature is raised to 327 C?
Q3)A gas mixture with a total pressure of 770 mmHgcontains each of the following gases at the indicated partial pressures: 120 mmHg CO2, 227mmHg Ar, and 190 mmHg O2. The mixture also contains helium gas
-What mass of helium gas is present in a 14.0-L sample of this mixture at 282 K ?
Q4)
A
Calculate the density of oxygen, O2, under each of the following conditions:
STP
1.00 atm and 35.0 C
Express your answers numerically in grams per liter. Enter the density at STP first and separate your answers by a comma.
B
To identify a diatomic gas (X2), a researcher carried out the following experiment: She weighed an empty 4.1-L bulb, then filled it with the gas at 2.00 atm and 24.0 C and weighed it again. The difference in mass was 9.5 g . Identify the gas.
Express your answer as a chemical formula.
Explanation / Answer
1- V1=V2=22.4l, P1=1atm , T1=273K , T2 =304K
P1V1/T1 = P2V2 /T2
P2= P1xT2/T1 = 1x304 /273 =1.11355atm
2-V1=V2=1.69L
P1=1.37 T1 = 273+17=290K, T2 = 273+327 = 600K
P2V2/T2 = P1V1/T1
P2 = P1 xT2 / T1 = 1.37 x 600 /290 =2.8345 atm
3-p total= 770mm
pCO2 =120mm , p Ar = 227mm, pO2 = 190
ptotal = pCo2 + pAr + pO2 + pHe
pHe = 770 - 537 = 233= 0.3066atm
PV = nRT
n= PV /RT = 0.3066 x14/282x0.082 = 4.2924/23.124 = 0 .1856
mass of He = nxMw = 0.1856x4=0.7425g
4-density O2 at STP
1 mole. of O2 = 32g.
1 mole. = 22.4L. at STP
Density = Mass / Volume.
Density of O2 at STP = 32g / 22.4L = 1.43g/L = 1.43kg/m³
P2 = 1atm T2 = 273+35= 308
V2 =?
P1V1/T1 = P2V2/T2
V2 = P1V1xT2/T1 P2=1x22.4 x308 /273x1 = 22.4x1.1282= 25.27
density= mass/volume = 32 / 25.27 = 1.2663g/L
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