Question

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=

Homework Answers

Answer #1

CH4 gives 1CO2 and 2H2O , total 3 gas molecules per 1CH4

C5H12 gives 5CO2 and 6H2O total 11 gas molecules per 1C5H12

Initially P = 0.5015 atm , we use PV = nRT equation

0.5015 x V = ( n1+ n2) x RT ................(1) where CH4 moles = n1 , C5H12 moles = n2

after combustion P = 2.421 atm , hence

2.421 x V = ( 3n1+ 11n2) x RT .....(2)

now ( 2/1)gives 2.421/0.5015 = ( 3n1+ 11n2) / ( n1+n2)

4.8275n1 + 4.8275 n2 = 3n1+11n2

1.8275 n1 = 6.1725 n2     hence n2 = 0.296 n1

mol fraction of CH4 = n1 / ( n1+n2) = n1 / ( n1+0.296n1) = n1 / ( 1.296) n1 = 0.7716

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
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.
A 5.00 g mixture of methane (CH4) and ethane (C2H6) is combusted in oxygen gas to...
A 5.00 g mixture of methane (CH4) and ethane (C2H6) is combusted in oxygen gas to produce carbon dioxide and water. If 14.09 g of CO2 is produced, how many grams of methane was in the original 5.00 g mixture ?
Pentane gas, C5H12 undergoes combustion with oxygen gas to produce carbon dioxide and water gases. a....
Pentane gas, C5H12 undergoes combustion with oxygen gas to produce carbon dioxide and water gases. a. Write the balanced chemical equation. b. How many grams of C5H12 are needed to produce 72 g of water? c. How many grams of CO2 are produced from 32.0 g of O2" please type and explain how you got the answer
When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The...
When methane (CH4) burns, it reacts with oxygen gas to produce carbon dioxide and water. The unbalanced equation for this reaction is CH4(g)+2O2(g)→CO2(g)+2H2O.What mass of carbon dioxide is produced from the complete combustion of 4.50×10−3 g of methane?
Problem Page Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide...
Problem Page Gaseous methane CH4 reacts with gaseous oxygen gas O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O . If 4.66g of carbon dioxide is produced from the reaction of 8.66g of methane and 24.2g of oxygen gas, calculate the percent yield of carbon dioxide. Be sure your answer has the correct number of significant digits in it.
2.In a mixture of helium, He, oxygen, 02, and methane, CH4, the partial pressures of helium...
2.In a mixture of helium, He, oxygen, 02, and methane, CH4, the partial pressures of helium and oxygen are 13.6 kPa and 29.2 kPa, respectively, and the total pressure if 95.4 kPa. The temperature of this mixture is 30°C. a)What is the partial pressure of methane? b)Methane undergoes a combustion reaction with oxygen to produce carbon dioxide and water. The UNBALANCED reaction is: c)If mixture described above is ignited and then cooled back to the original temperature of 30°C, what...
Methane (CH4) and oxygen (O2) react in the presence of a catalyst to give formaldehyde (HCHO)....
Methane (CH4) and oxygen (O2) react in the presence of a catalyst to give formaldehyde (HCHO). In a parallel reaction the methane is oxidized to carbon dioxide and water: CH4 + O2 → HCHO + H2O CH4 + 2O2 → CO2 + 2H2O The feed to the reactor contains equimolar amounts of methane and oxygen. Assume as a base a feed of 100 mol / s. The methane conversion fraction is 0.90 and the yield fraction of formaldehyde is 0.855....
When methane (CH4) burns it combines with oxygen and forms carbon dioxide and water. Which of...
When methane (CH4) burns it combines with oxygen and forms carbon dioxide and water. Which of the following is the balanced chemical reaction for the burning of methane? CH4 + O2 → CO2 + H2O 3 CH4 + 6 O2 → 3 CO2 + 6 H2O 2 CH4 + 3 O2 → CO2 + 4 H2O CH4 + 3 O2 → 2 CO2 + 2 H2O CH4 + 2 O2 → CO2 + 2 H2O
Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and...
Gaseous methane (CH4) reacts with gaseous oxygen gas (O2) to produce gaseous carbon dioxide (CO2) and gaseous water (H2O). If 2.59g of water is produced from the reaction of 6.58g of methane and 14.4g of oxygen gas, calculate the percent yield of water. Be sure your answer has the correct number of significant digits in it.
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 %...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT