Question

what is the mass in kg of CO2 formed by combusting enough fuel to release 1.0...

what is the mass in kg of CO2 formed by combusting enough fuel to release 1.0 kJ of energy for this equation?

CH4 + 2O2 -> CO2 + 2H2O

Homework Answers

Answer #1

CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)

Hrxn = H0f products - H0f reactants

             = 2*-285.83-393.5 -(-74.81+2*)

              = -890.35KJ/mole

CH4(g) + 2O2(g) -> CO2(g) + 2H2O(l)      Hrxn = -890.35KJ/mole

1 mole of CO2 produce to released -890.35KJ

-890.35 Kj energy is released from 1 mole of CO2

-890.35 Kj energy is released from 44g of CO2

1KJ energy is released from = 44*1/890.35   = 0.05g of CO2

0.05g of CO2= 5*10^-2 g of CO2

                          = 5*10^-5Kg of CO2>>>>>answer

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
what is the mass in kg of CO2 formed by combusting enough fuel to release 1.0...
what is the mass in kg of CO2 formed by combusting enough fuel to release 1.0 kJ of energy for this equation? C3H8 + 5O2 -> 3CO2 + 4H2O
Part A Determine the mass of CO2 produced by burning enough of methane to produce 2.25×102kJ...
Part A Determine the mass of CO2 produced by burning enough of methane to produce 2.25×102kJ of heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ Express your answer using three significant figures. Part B Determine the mass of CO2 produced by burning enough of propane to produce 2.25×102kJ of heat. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2217kJ Express your answer using three significant figures. Part C Determine the mass of CO2 produced by burning enough of octane to produce 2.25×102kJ of heat. C8H18(l)+25/2O2(g)→8CO2(g)+9H2O(g)ΔH∘rxn=−5074.1kJ Express your answer using three significant figures. Part D...
Part A Determine the mass of CO2 produced by burning enough of methane to produce 1.00×102kJ...
Part A Determine the mass of CO2 produced by burning enough of methane to produce 1.00×102kJ of heat. CH4(g)+2O2(g)→CO2(g)+2H2O(g)ΔH∘rxn=−802.3kJ Express your answer using three significant figures. Part B Determine the mass of CO2 produced by burning enough of propane to produce 1.00×102kJ of heat. C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2217kJ Express your answer using three significant figures. Part C Determine the mass of CO2 produced by burning enough of octane to produce 1.00×102kJ of heat. C8H18(l)+25/2O2(g)→8CO2(g)+9H2O(g)ΔH∘rxn=−5074.1kJ Express your answer using three significant figures.
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
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
CO2 intensity: Per kilogram of fuel combusted, the following fuels release the following amounts of energy:...
CO2 intensity: Per kilogram of fuel combusted, the following fuels release the following amounts of energy: butane (C4H10), 50 MJ; wood (CH2O), 10 MJ; gasoline (C8H18), 50 MJ; coal (pure carbon), 30 MJ. Calculate the energy released per kilogram of CO2 emitted for these fuels.
1. What is the final concentration when 475 mL of 6.0 M HCl solution is diluted...
1. What is the final concentration when 475 mL of 6.0 M HCl solution is diluted to a final volume of 1.45 L? 2. A gas has a volume of 675 mL at 308 K and 646 mmHg pressure. What is the volume (L) of the gas at −95°C and a pressure of 1.06 atm (n is constant)? 3. Find out the number of molecules present in 2.54g of copper (I) chloride. 4. Determine the limiting reactant for the following...
A large SUV has a mass of 2700 kg. Calculate the mass of CO2 emitted into...
A large SUV has a mass of 2700 kg. Calculate the mass of CO2 emitted into the atmosphere upon accelerating the SUV from 0.0 to 63.0 mph . Assume that the required energy comes from the combustion of octane (ΔH∘f=−250.1 kJ) with 30% efficiency.
Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in...
Charcoal is primarily carbon. What mass of CO2 is produced if you burn enough carbon (in the form of charcoal) to produce 4.90kJ×102kJ of heat? The balanced chemical equation is as follows: C(s)+O2(g)→CO2(g),ΔH∘rxn=−393.5kJ Express the mass in grams to three significant figures.
A) If 30.8 g of O2 are mixed with 30.8 g of H2 and the mixture...
A) If 30.8 g of O2 are mixed with 30.8 g of H2 and the mixture is ignited, what mass of water is produced? B) Iron is produced from its ore by the reactions: 2C(s)+O2(g) → 2CO(g) Fe2O3(s)+3CO(g) → 2Fe(s) + 3co2(g) How many moles of O2(g) are needed to produce 9.5 moles of Fe(s)? C) Which of the following equations correctly describes the combustion of CH4and O2to produce water (H2O) and carbon dioxide (CO2)? a)     CH4 + O2 ...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT