Question

LP gas burns according to the following exothermic reaction: C3H8(g)+5O2(g)→3CO2(g)+4H2O(g)ΔH∘rxn=−2044kJ What mass of LP gas is necessary to heat 1.5 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

Answer #1

find ot the fist mass of water

1.5L means 1500 ml since density of water = 1, 1 ml = 1 graso 1500 ml = 1500 gr

heat abosrbed by water = m x c x delta T

m = mass of the water = 1500 gr

c - specific heat of the water = 4.184 J/g ºC

delta T = T2-T1 = 100-75

put all these in the above equation

heat abosrbed by water = 1500 g x 4.184 J/g ºC x (100 ºC-25 ºC) = 471,000 J = 471 kJ

471 kJ x (1 mole C3H8 / 2044 kJ) x (44.0 g C3H8 / 1 mole C3H8) = 10.1 g C3H8

Since it is only 14% efficient,

10.1 g C3H8 x (100 / 14) = 72.143 g C3H8.

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.

Consider the combustion reaction of propane gas: C3H8(g) +
5O2(g) → 4H2O(g) + 3CO2(g) Predict the signs (+ positive, -
negative, 0 zero, or CBD cannot be determined ), if possible, for
the delta Ssystem. Use the symbol to fill the blank.

Given the following balanced reaction: C3H8(g) + 5O2(g) →
3CO2(g) + 4H2O(g)
A.) Given 7.65 kg of C3H8 and 3.14 kg of O2,determine the
limiting reagent
B.)Determine the number of moles of CO2 produced
C.)Determine the number of kg of CO2 produced
D.)Determine the number of kg of excess reagent left
E.)Given that only 1.88 kg of CO2 are actually produced what is
the percent yeild?

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...

18. Butane gas burns according to the following exothermic
reaction:
C4H10 (g) + 13/2 O2 (g) → 4 CO2 (g) + 5 H2O (g) ∆H°rxn = -
2877.1 kJ
a) If 25.0 g of butane were burned, how much energy would be
released?
b) If the reaction of 25.0 g of butane produced a volume change
of 15.4 L against an external pressure of 748 mmHg, calculate the
work done (in J).
c) Calculate the change in internal energy (∆E)...

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

Which of the following is an acid based reaction?
Pb(NO3)2+2KI->2KNO3+PbI2
2Mg+O2->2MgO
C2H8+5O2->3CO2+4H2O
H2SO4+2KOH->K2SO4+2H2O
Place the correct coefficients to balance the reaction
below:
____CH4 + ____O2→
____CO2 + ____H2O_____
H2CO3 --> H2O +
CO2 is a
Decomposition reaction
Single replacement reaction
Combustion Reaction
Synthesis Reaction
Double replacement reaction
Balance the following reaction
___Al + ___O2→
___Al2O3
2,1,1
4,3,2
2,3,1
5,3,2
Mg + 2HCI->MgCI+H2
How many grams of H2 will be produced from 12 grams of Mg
3.0
2.0
1.0
4.0
Balance...

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