If 646 L of gaseous ethanol reacts with 161 L O2 what is the

If 6.46 L of gaseous ethanol reacts with 16.1 L O₂, what is the maximum volume of gaseous carbon dioxde produced? Assume that the temperature of the reactants and products is 425 °C and the pressure remains constant at 1.00 atm.
CH₃CH₂OH(g) + 3 O₂(g) ® 2 CO₂(g) + 3 H₂O(g)

6.46 L
10.7 L
12.9 L
16.1 L
22.6 L

2.

At what temperature does 742 mm Hg of CH₄ gas have the same density as 742 mm Hg of O₂ gas at 273 K?

137 K
146 K
191 K
275 K
545 K

3.
A 10.0 L flask at 318 K contains a mixture of Ar and CH₄ with a total pressure of 1.040 atm. If the mole fraction of Ar is 0.715, what is the mass percent of Ar?

13.8%
68.8%
71.5%
82.9%
86.2%

4. Methane gas, CH₄, effuses through a barrier at a rate of 0.568 mL/minute. If an unknown gas effuses through the same barrier at a rate of 0.343 mL/minute, what is the molar mass of the gas?

20.8 g/mol
28.0 g/mol
32.0 g/mol
44.0 g/mol
64.0 g/mol

5. Carbon monoxide reacts with oxygen to form carbon dioxide.
2 CO(g) + O₂(g) ® 2 CO₂(g)
In a 1.00 L flask, 4.30 atm of CO reacts with 2.50 atm of O₂. Assuming that the temperature remains constant, what is the final pressure in the flask?

1.80 atm
2.50 atm
4.30 atm
4.65 atm
6.80 atm

Solution

1)from stoichoimetry,and as P&T remains constant

volume of Co2=12.92 litres

2)pv=nrt

n/v=p/RT

m/v=pM/RT

742*16/RT= 742*32/R*273

T=136.5K=137K

3)PV=NRT

1.040*10=0.0821*N*318

N=0.3983

mole of Ar=0.2848

moles of CH4=0.1135

so mass % of Ar= 0.2848*40/(0.2848*40 +0.1135*16) =86.25%

4)0.568/0.343=sqrt(M/16)

M=43.876=44

5)

O2 is limiting

so O2 consumed=2.15 atm

co O2 remaining=0.35 atm

CO2 produced=4.3 atm

so total pressure=4.3+.35=4.65 atm