Question

15. Consider the following combustion reaction of propane. 3C3H8
+ 5O2 → 3CO2 + 4H2O

a) What mass of O2 , in g, would be needed to react with 0.421 kg
of C3H8?

b) What mass of CO2 , in g, would be produced from the combustion
of 0.421 kg of C3H8 with excess oxygen?

Answer #1

**A)
mass of C3H8 = 0.421 kg = 421 g
molar mass of C3H8 = 44.094 g/mol
mol of C3H8 = (mass)/(molar mass)
= 421/44.094
= 9.547784 mol
According to balanced equation
mol of O2 required = (5/3)* moles of C3H8
= (5/3)*9.547784
= 15.912974 mol
mass of O2 = number of mol * molar mass
= 15.912974*32
= 509 g
= 0.509 Kg
Answer: 0.509 Kg**

**B)
According to balanced equation
mol of CO2 formed = moles of C3H8
= 9.55 mol
mass of CO2 = number of mol * molar mass
= 9.55*44.01
= 420 g
= 0.420 Kg
Answer: 0.420 Kg**

Consider the Combustion of Propane (C3H8)by O2 and H2o.
C3H8
+5O2 --> 3Co2+ 4H2o
D) At standard temperature and pressure, what
volume of oxygen would be required to burn 100 g of propane? If air
is 21 percent oxygen, what volume of air at STP would be
required?
E) At standard temperature and pressure, what volume of Co2
would be produced when 100g of propane are burned?

Consider the balanced equation for the combustion of propane,
C3H8 C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l) If propane reacts with
oxygen as above a. what is the limiting reagent in a mixture
containing 5.00 g of C3H8 and 10.0 g of O2? b. what mass of the
excess reagent remains after the reaction ? c. what mass of CO2 is
formed when 1.00 g of C3H8 reacts completely?

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?

C3H8 (l) + 5O2 (g) → 3CO2 (g) + 4H2O (l)
A)How much work is done at 1.2 atm and 334 K when 1 mole of
propane undergoes combustion?
B)How much work is done at 1.2 atm and 310 K when 102 grams of
oxygen reacts with excess propane in this combustion reaction.?

1. The combustion of methane can be
written as: C3H8 + 5O2 ==
3CO2 + 4H2O. Determine (a) the theoretical
combustion air, (b) the excess combustion air at 100% excess rate,
and (c) the actual combustion air. Report the amount per lb-mole of
C3H8 and per lb of
C3H8.

#6 The following reaction shows combustion reaction of propane
gas at 25 Celsius.
C3H8(gas)+5O2(gas)<===>
3CO2(gas)+4H20(liq);
deltaH=-2219.97 kJ/mol
Initially 1L-chamber contained 2.03M of propane
(C3H8), 3.50 M of oxygen (O2) and
0.030M of carbon dioxide (CO2). After equilibrium is
reached, the chamber contained 1.53 M of propane
(C3H8).
a)Using the information given,calculate equlibrium constant
(Kc) of thid reaction.
b) After equilibrium is reached, if the chamber size is
increased to 5L, predict the direction of equilibrium shift.
Explian your answer.
c)After...

Calculate ΔSuniv (in kJ/K mol) for the combustion of propane at
25 °C. C3H8(g) 5O2(g) --> 3CO2(g) 4H2O(g)

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

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.

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