Question

**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*)Δ*H*∘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*)Δ*H*∘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*)Δ*H*∘rxn=−5074.1kJ

Express your answer using three significant figures.

**Part D**

Which fuel contributes least to global warming per kJ of heat produced?

propane |

methane |

octane |

Answer #1

Solution:- According to the given data

1) The reaction is as follows

Here, 1 mole of.. is produced from 1 mole of...

In this process the amount of heat .. is released for the 1 mole of....

Here calculate the mass of CO_{2} is produced.

Here calculate the mass of CO_{2} produced to
release

ii) The reaction is as follows

Here, 3 mole of CO_{2} produced from 1 mole....

Tn this process the amount of heat 2217 kj released for 3 mole
of CO_{2} is produced.

In this process the amount of heat 5074.1 KJ is released for 8 mole .....

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.

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) Butane combusts according to the equation: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g)
ΔHrxn=−2658kJ
- What mass of butane in grams is
necessary to produce 1.1×103 kJ kJ of heat? Express your answer to two significant figures
and include the appropriate units.
- What mass of CO2 is
produced? Express your answer
to two significant figures and include the appropriate
units.
B) Charcoal is primarily carbon. What mass of CO2
is produced if you burn enough carbon (in the form of charcoal) to
produce 5.10×102kJ...

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

Question 4
Part A
Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 → 16
CO2 + 18 H2O ΔH°rxn = -11018
kJ
Using the following equation for the combustion of octane,
calculate the heat of reaction for 100.0 g of octane. The molar
mass of octane is 114.33 g/mole.
2 C8H18 + 25 O2 → 16...

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine
ΔSuniv.
Part A
ΔH∘rxn=− 89 kJ , ΔSrxn=− 150 J/K , T= 310 K
Express your answer using two significant figures.
Part B
ΔH∘rxn=− 89 kJ , ΔSrxn=− 150 J/K , T=
758 K
Express your answer using one significant figure.
Part C
ΔH∘rxn=+ 89 kJ , ΔSrxn=− 150 J/K , T=
310 K
Express your answer using two significant figures.
Part D
ΔH∘rxn=− 89 kJ , ΔSrxn=+ 150 J/K...

Part A
For which of the following reactions is ΔH∘rxn equal to
ΔH∘f of the product(s)?
You do not need to look up any values to answer this
question.
Check all that apply.
Hints
Check all that apply.
S(s)+O2(g)→SO2(g)
Li(s)+12F2(g)→LiF(s)
SO(g)+12O2(g)→SO2(g)
SO3(g)→12O2(g)+SO2(g)
2Li(s)+F2(g)→2LiF(s)
Li(s)+12F2(l)→LiF(s)
Part B
The combustion of propane, C3H8, occurs via the reaction
C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)
with heat of formation values given by the following table:
Substance
ΔH∘f
(kJ/mol)
C3H8 (g)
-104.7
CO2(g)
−393.5
H2O(g)
−241.8
Calculate the enthalpy for...

Liquefied petroleum (LP) gas burns according to the following
exothermic reaction:
C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2044kJ
.
Part A
What mass of LP gas is necessary to heat 1.8 L of water from
room temperature (25.0 ∘C) to boiling (100.0 ∘C)? Assume that,
during heating, 14% of the heat emitted by the LP gas combustion
goes to heat the water. The rest is lost as heat to the
surroundings.
Express your answer using two significant figures.

Gaseous methane CH4 will react with gaseous oxygen O2 to produce
gaseous carbon dioxide CO2 and gaseous water H2O . Suppose 11. g of
methane is mixed with 73.5 g of oxygen. Calculate the maximum mass
of water that could be produced by the chemical reaction. Round
your answer to 2 significant digits.

Gaseous methane CH4 will react with gaseous oxygen O2 to produce
gaseous carbon dioxide CO2 and gaseous water H2O
. Suppose 3.05 g of methane is mixed with 8.0 g of oxygen.
Calculate the maximum mass of water that could be produced by the
chemical reaction. Be sure your answer has the correct number of
significant digits.

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