Question

Nitromethane (CH3NO2) burns in air to produce significant amounts of heat.

2CH3NO2(l)+(3/2)O2(g)→ 2CO2(g)+3H2O(g)+N2(g)

ΔH∘rxn=−1418kJ

How much heat is produced by the complete reaction of 5.02 kg of nitromethane?

Express your answer with the appropriate units.

q = ??

Answer #1

Nitromethane (CH3NO2) burns in air to produce significant
amounts of heat. 2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g) ΔHorxn =
-1418 kJ How much heat is produced by the complete reaction of 4.35
kg of nitromethane?

Nitromethane (CH3NO2) burns in air to produce significant
amounts of heat. 2CH3NO2(l)+3/2O2(g)→2CO2(g)+3H2O(l)+N2(g) ΔHrxn =
-1418 kJ How much heat is produced by the complete reaction of 7.68
kg of nitromethane?

Calculate ΔH∘rxn. C2H5OH(l)+3O2(g)→2CO2(g)+3H2O(g) Express your
answer using five significant figures.

C2N2O2Hg(s) + O2 (g)
-> Hg(g) + 2CO2(g) + N2(g)
Determine the theoretical enthalpy (in kJ/mol) of the mercury
fulminate reaction by using the enthalpy of formation for mercury
fulminate (+ 386 kJ/mol) Remember, ΔH° rxn = Σn x
H°f(products) - Σn x ΔH°f(reactants). Explain
your work. We are assuming a constant pressure situation.
This is can also be termed the heat of
explosion, but when it is termed heat of explosion,
the units are traditionally kJ/kg of substance. Convert...

From the enthalpies of reaction
2H2(g)+O2(g)→2H2O(g)ΔH=−483.6kJ3O2(g)→2O3(g)ΔH=+284.6kJ calculate
the heat of the reaction 3H2(g)+O3(g)→3H2O(g) Express your answer
using four significant figures. I have no idea how to approach this
problem.

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

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.

The standard heat of formation, ΔH∘f, is defined as the enthalpy
change for the formation of one mole of substance from its
constituent elements in their standard states. Thus, elements in
their standard states have ΔH∘f=0. Heat of formation values can be
used to calculate the enthalpy change of any reaction.
Consider, for example, the reaction
2NO(g)+O2(g)⇌2NO2(g)
with heat of formation values given by the following table:
Substance ΔH∘f
(kJ/mol)
NO(g) 90.2
O2(g) 0
NO2(g) 33.2
Then the standard heat...

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...

Part C
Calculate the molar mass of acetylcholine (C7NH16O2), a
neurotransmitter that activates muscles.
Express your answer to five significant figures.
Molar mass =
g/mol
Calculate the number of moles in 3.47 g of each of the
following:
Part A
He
Express your answer with the appropriate units. n=
Part B
SnO2
Express your answer with the appropriate units. n=
Part C
Cr(OH)3
Express your answer with the appropriate units. n=
Part D
Ca3N2
Express your answer with the appropriate...

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