Question

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

Homework Answers

Answer #1

Note 101.325 J/atm-L is conversion factor to convert atm-L to J.

Comment in case of any doubt.

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
Consider the following chemical reaction: CH4 + 2O2 → CO2 + 2H2O 4 moles of methane...
Consider the following chemical reaction: CH4 + 2O2 → CO2 + 2H2O 4 moles of methane (CH4) are combined with 5 moles of oxygen (O2). How much carbon dioxide (CO2) will form?
The two competing reactions for the combustion of methane in a combustor are: CH4 + 2O2...
The two competing reactions for the combustion of methane in a combustor are: CH4 + 2O2 ? CO2 + 2H2O and CH4 + 3/2 O2 ? CO + 2H2O The feed to the combustor contains 7.8 mol% CH4, 19.4% O2, and 72.8% N2 and the gas leaving the reactor contains 8 mol CO2/mol CO. Using a basis of 100 mol/h of feed to the reactor. 1) If 100 mol/h of CH4 is fed to the combustor, i). what is the...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of...
The combustion of methane, CH4, releases 890.4 kj/mol of heat. That is, when one mole of methane is burned, 890.4 kj are give off to the surroundings. This means that the products have less energy stored in the bonds than the reactants. Thus, for the reaction: CH4(G) + 2 O (g) -> CO2 (g) + 2 H2O (I) deltaH= -890.4kj/mol. A) what is the enthalpy change when 2.00 mol of CH4 are burned? B)what is the enthalpy change when 22.4g...
The gas methane, CH4(g), can be used in welding. When methane is burned in oxygen, the...
The gas methane, CH4(g), can be used in welding. When methane is burned in oxygen, the reaction is: CH4(g) + 2 O2(g)------>CO2(g) + 2 H2O(g)      (a) Using the following data, calculate ^H° for this reaction. ^H°f kJ mol-1:   CH4(g) = -74.6 ; CO2(g) = -393.5 ; H2O(g) = -241.8 ^H° = _____ kJ (b) Calculate the total heat capacity of 1 mol of CO2(g) and 2 mol of H2O(g), using CCO2(g) = 37.1 J K-1 mol-1 and CH2O(g) =...
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?
Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l)...
Calculate the ΔH∘ for this reaction using the following thermochemical data: CH4(g)+2O2(g)⟶CO2(g)+2H2O(l) ΔH∘=−890.3kJ C2H4(g)+H2(g)⟶C2H6(g) ΔH∘=−136.3kJ 2H2(g)+O2(g)⟶2H2O(l) ΔH∘=−571.6kJ 2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l)
What mass of natural gas (CH4) must you burn to emit 275 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ...
What mass of natural gas (CH4) must you burn to emit 275 kJ of heat? CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ m = Pentane (C5H12) is a component of gasoline that burns according to the following balanced equation: C5H12(l)+8O2(g)→5CO2(g)+6H2O(g) Part A Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. (The standard enthalpy of formation of liquid pentane is -146.8 kJ/mol.) Express your answer using five significant figures. ΔH∘rxn = kJ
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....
Calculate ΔH° for the combustion of methane (products are CO2(g) and H2O(l)), given the following thermochemical...
Calculate ΔH° for the combustion of methane (products are CO2(g) and H2O(l)), given the following thermochemical equations: CH4(g) + O2(g) →CH2O(g) + H2O(g) ΔH = -284 kJ CH2O(g) + O2(g) →CO2(g) + H2O(g) ΔH = -518 kJ H2O(g) →H2O(l) ΔH = +44 kJ
A sample of gas contains 0.1400 mol of CH4(g) and 0.2800 mol of O2(g) and occupies...
A sample of gas contains 0.1400 mol of CH4(g) and 0.2800 mol of O2(g) and occupies a volume of 14.9 L. The following reaction takes place: CH4(g) + 2O2(g)CO2(g) + 2H2O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. ______L