Question
At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8)...
At 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C3H8) was burned, producing 15.7 g of CO2. What was the mole fraction of each gas in the mixture? Assume complete combustion.
Homework Answers
Answer #1
Not the answer you're looking for?
Similar Questions
A closed container has a mixture of methane, CH4, ethane, C2H6, and propane, C3H8. If 26.5...
A closed container has a mixture of methane, CH4,
ethane, C2H6, and propane,
C3H8. If 26.5 g of methane, 29.5 g of ethane,
and 31.0 g of propane are placed in the 8.60 L container at 58.5°C,
what is the total pressure in the container? Assume the gases do
not react with each other.
atm
A closed container has a mixture of methane, CH4, ethane, C2H6, and propane, C3H8. If 17...
A closed container has a mixture of methane, CH4, ethane, C2H6,
and propane, C3H8. If 17 g of methane, 21.6 g of ethane, and 30.3 g
of propane are placed in the 4.74 L container at 63.7°C, what is
the total pressure in the container (in atm)? Assume the gases do
not react with each other
When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00 atm, H2O (l)...
When 1.000 g of propane gas (C3H8) is burned at 25ºC and 1.00
atm, H2O (l) and CO2 (g) are formed with the evolution of 50.33 kJ
of energy.
Substance
∆Hºf (kJ mol -1)
Sº (J mol -1 K -1)
H2O (l)
- 285.8
69.95
CO2 (g)
- 393.5
213.7
O2 (g)
0.0
205.0
C3H8 (g)
?
270.2
Calculate the molar enthalpy of combustion, ∆Hºcomb , of propane
and the standard molar enthalpy of formation, ∆Hºf , of propane
gas.
A gaseous fuel mixture stored at 736 mm Hg and 298 K contains only methane (CH4)...
A gaseous fuel mixture stored at 736 mm Hg and 298 K contains
only methane (CH4) and propane
(C3H8). When 11.0 L of this fuel mixture is
burned, it produces 722 kJ of heat. What is the mole fraction of
methane in the mixture? (Assume that the water produced by the
combustion is in the gaseous state.)
A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has a pressure of 0.5015 atm...
A mixture of methane gas, CH4(g), and pentane gas, C5H12(g), has
a pressure of 0.5015 atm when placed in a sealed container. The
complete combustion of the mixture to carbon dioxide gas, CO2(g),
and water vapor, H2O(g), was achieved by adding exactly enough
oxygen gas, O2(g), to the container. The pressure of the product
mixture in the sealed container is 2.421 atm. Calculate the mole
fraction of methane in the initial mixture assuming the temperature
and volume remain constant. Xch4=
Consider the balanced equation for the combustion of propane, C3H8 C3H8(g) + 5O2(g) 3CO2(g) +...
Consider the balanced equation for the combustion of propane,
C3H8 C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) If propane reacts with
oxygen as above a. what is the limiting reagent in a mixture
containing 5.00 g of C3H8 and 10.0 g of O2? b. what mass of the
excess reagent remains after the reaction ? c. what mass of CO2 is
formed when 1.00 g of C3H8 reacts completely?
A particular natural gas consists, in mole percents, of 83.0% CH4 (methane), 11.2% C2H6 (ethane), and...
A particular natural gas consists, in mole percents, of 83.0%
CH4 (methane), 11.2% C2H6 (ethane), and 5.80% C3H8 (propane). A
385-L sample of this gas, measured at 25 ∘C and 729 mmHg , is
burned in an excess of oxygen gas.
How much heat, in kilojoules, is evolved in this
combustion reaction?
Express your answer with the appropriate
units.
The table shown here gives the enthalpy of combustion for three
different hydrocarbon fuels to produce liquid water and gaseous
carbon...
the combustion of methane, CH4, in oxygen. CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l) the...
the combustion of methane, CH4, in oxygen.
CH4(g) + 2O2(g) >> CO2(g) + 2H2O (l)
the heat of reaction at 77C and 1.00 atm is -885.5 kJ. what is
the change in volume when 1.00 mol CH4 reacts with 2.00 mol O2.
what is w for this change?
calculate delta U (change in U) for the change indicated by the
chemical equation
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and
an unknown amount of propane, C3H8) were added to the same 10.0-L
container. At 23.0 ∘C, the total pressure in the container is 4.40
atm . Calculate the partial pressure of each gas in the container.
Express the pressure values numerically in atmospheres, separated
by commas. Enter the partial pressure of methane first, then
ethane, then propane. A gaseous mixture of O2 and N2 contains 37.8
%...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and an unknown amount...
Three gases (8.00 g of methane, CH4, 18.0 g of ethane, C2H6, and
an unknown amount of propane, C3H8) were added to the same 10.0-L
container. At 23.0 ∘C, the total pressure in the container is 5.30
atm . Calculate the partial pressure of each gas in the
container.
ADVERTISEMENT
Need Online Homework Help?
Get Answers For Free
Most questions answered within 1 hours.
ADVERTISEMENT
Active Questions
asked 11 minutes ago
asked 27 minutes ago
asked 29 minutes ago
asked 31 minutes ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 1 hour ago
asked 2 hours ago