Question

The combustion of 1 gram of natural gas releases 50.1kJ of heat.

Calculate the mass of co2 released when natural gas is burnt to produce 1500 kJ od heat. Natural gas is assumed to be pure methane: CH4

Answer: The mass of co2 produced when natural gas (CH4) was used as fuel came out to be 82 grams.

Question: What would be the value of co2 produced if Bituminous coal (C135H96O9NS) is used to produce the same 1500 kJ of heat?

Answer #1

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?

Methane gas at 400K and 1 atm enters a combustion chambar where
it is mixed with air entering at 500K, 1 atm. The products of
combustion exit at 1800K and 1 atm with product analysis given
in
For operation at steady state, determine the rate of the heat
transfer from the combustion chamber in kJ/kmol of fuel. Neglect
kinetic and potential energy effect . The average value for the
specific heat of methane between 298 and 400K is 38kJ/molK. The...

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...

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

3. Fossil fuels (petroleum, natural gas, and coal) are excellent
fuels composed primarily of hydrocarbons, which when burned in an
adequate supply of air are oxidized, forming carbon dioxide and
water. Chemical bonds are broken and new bonds are formed, and as a
result, energy is released as heat. Calculate the following in the
spaces provided using the table below. Show all work.
Hydrocarbon
Heat of Combustion (kJ/g)
Molar Heat of Combustion (kJ/mol)
Methane
55.6
890
Ethane
52
1560
Propane...

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) =...

Constants | Periodic Table
The coefficients in a balanced chemical equation provide the
mole-to-mole stoichiometry among the reactants and products. The
molar mass (in g/mol) can be used as the conversion factor between
moles and the mass of a substance. Thus, the balanced equation and
molar masses can be used in conjunction with one another to
calculate the masses involved in a reaction.
Complete combustion of methane
When methane (CH4) burns, it reacts with oxygen gas to produce
carbon dioxide...

± Stoichiometric Relationships with Gases
The ideal gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant Requals 0.08206 L⋅atm/(K⋅mol) or 8.3145
J/(K⋅mol). The equation can be rearranged as follows to solve for
n:
n=PVRT
This equation is useful when dealing with gaseous reactions because
stoichiometric calculations involve mole ratios.
Part A
When heated, calcium carbonate decomposes to yield calcium oxide
and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)...

The ideal gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant Requals 0.08206 L⋅atm/(K⋅mol) or 8.3145
J/(K⋅mol). The equation can be rearranged as follows to solve for
n:
n=PVRT
This equation is useful when dealing with gaseous reactions
because stoichiometric calculations involve mole ratios.
A)When heated, calcium carbonate decomposes to yield calcium
oxide and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)
What is the mass of calcium carbonate...

1. Calculate the thermoeconomic cost of the produced electricity
using the internal combustion device described in homework 7. with
and without the heat exchanger. Use the results you calculated to
answer this question. This question is focusing on the
thermoeconomic costs. The electricity is produced for 10 hours a
day, five days per week during a one year cycle.
The following cost information is given for the internal
combustion device. The cost of the device is $125,000 and it has...

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