1. What volume of Cl2(g) at STP would you need to obtain a 250g sample of Cl2(g)?
3. What is the volume, in liters, occupied by a mixture of 15.2g Ne(g) and 34.8g Ar(g) at 7.15 atm pressure and 26.7 degrees Celsius?
4. An 89.3mL sample of "wet" 02(g) is collected over water at 21.3 degrees Celsius at a barometric pressure of 756mmHg (vapor pressure of water at 21.3 degree Celsius = 19mmHg)
a. What is the partial pressure of 02(g) in millimeters of mercury in the sample collected.
b. What is the volume percent O2 in the gas collected?
c. How many grams of O2 are present in the sample?
5. Calculate the volume of H2(g) measured at 26 degrees Celsius and 751 Torr required to react with 28.5 L CO(g), measured at 0 degree Celsius and 760 torr in the following reaction.
3 CO(g) + 7 H2(g) --- C3H8(g) + 3H20(l)
1. Assume Cl2 follow ideal gas law:
At STP conditions:
So you need the number of mole of Cl2
Molecular weight of Cl2=2*35.5=71(g/mol)
Number of mole of Cl2=250/71=3.52(mol)
Substitute into PV=nRT
2. Using PV=nRT
We can calculate ...
The solution provides detailed explanations and calculations for the problem.
1. Benzene is an organic solvent with the formula, C6H6. It boils at 80.1oC and melts at 5.5oC. Benzene's density is 0.88 gm/ml, its heat of vaporization is 20.0 KJoules per mole, its heat of fusion is 10.0 KJoules per mole, its heat capacity is 0.50 KJoules per mole-degree C for liquid benzene, 0.25 KJoules per mole-degree C for solid benzene, and 0.125 KJoules per mole-degree C for gaseous benzene.
Calculate the following:
1. The energy required to heat 390 grams of benzene from 150oC to 450o C.
2. The energy to removed heat 3.9 milligrams of benzene from 15oC to 60oC.
3. The energy removed to cool 390 kilograms of benzene from -70oC to -90oC.
4. The volume occupied by 1 micromole of liquid benzene and the volume occupied by 1 megamole of benzene as a vapor at STP (assume an ideal gas)
5. The energy required to cool 7.8 grams of benzene from -150oC to 400o C.