In: Chemistry
Q1)Aluminum reacts with chlorine gas to form aluminum chloride. 2Al(s)+3Cl2(g)→2AlCl3(s).What minimum volume of chlorine gas (at 298 K and 229 mmHg ) is required to completely react with 8.60 g of aluminum? please explain the step, how you got to the answer for this problem.
A)38.8 mL
B)38.8 L
C)388 L
D)0.388 L
Q2)Calculate the density of oxygen, O2 under each of the following conditions
STP and 1.00atm and 35.0 Celcius
(Express answer numerically in grams per liter. Enter density at STP first & seperate your answer by a comma)
Q3) To identify a diatomic gas(
X2), a researcher carried out the following experiment: She weighed an empty 4.3-Lbulb, then filled it with the gas at 1.90 atm and 23.0 ∘Cand weighed it again. The difference in mass was 9.5 g . Identify the gas.(Express answer as chemical formula)
Solution : -
Q1)Aluminum reacts with chlorine gas to form aluminum chloride. 2Al(s)+3Cl2(g)→2AlCl3(s).What minimum volume of chlorine gas (at 298 K and 229 mmHg ) is required to completely react with 8.60 g of aluminum?
Balanced reaction equation
2Al + 3Cl2 ----- > 2AlCl3
Now lets calculate the moles of 8.62 g Al
8.60 g Al * 1 mol /26.982 g per mol = 0.31873 mol Al
Now lets calculate moles of Cl2 using the moles of Al
0.31873 mol Al * 3 mol Cl2 / 2 mol Al = 0.4781 mol Cl2
Now lets calculate the volume of the Cl2 gas needed at the given conditions
PV= nRT
V= nRT/P
= 0.4781 mol * 0.08206 L atm per mol K * 298 K / (229 mmHg * 1 atm / 760 mmHg)
= 38.8 L
So the volume of Cl2 needed is 38.8 L
Q2)Calculate the density of oxygen, O2 under each of the following conditions
STP and 1.00atm and 35.0 Celcius
Formula to calculate the density is
PM= dRT
d=PM/RT
= 1 atm * 32.0 g per mol / 0.08206 L atm per mol K * (35.0 C +273 )
= 1.226 g/ L
So the density of the oxygen gas is 1.226 g / L
Solution :-
Lets first calculate the moles of the gas
P = 1.90 atm
T= 23.0 C +273 = 296 K
V = 4.3 L
PV= nRT
PV/RT = n
1.90 atm * 4.3 L / 0.08206 L atm per mol K * 296 K = n
0.33636 mol = n
Now using the moles and mass of the gas lets calculate its molar mass
Molar mass = mass / moles
= 9.5 g / 0.33636 mol
= 28.2 g per mol
So the diatomic gas is N2 because molar mass of N2 = 28.01 g per mol