Question

How many grams of octane (C8H18) are needed to produce 100.0 g of carbon dioxide in a complete combustion reaction if the reaction occurs with a 60.0% yield?

Answer #1

for CO2

% yield = actual mass*100/theoretical mass

60.0= 100*100/theoretical mass

theoretical mass = 166.7 g

Molar mass of CO2 = 1*MM(C) + 2*MM(O)

= 1*12.01 + 2*16.0

= 44.01 g/mol

mass of CO2 = 166.7 g

mol of CO2 = (mass)/(molar mass)

= 166.7/44.01

= 3.7878 mol

we have the Balanced chemical equation as:

2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O

From balanced chemical reaction, we see that

when 16 mol of CO2 forms, 2 mol of C8H18 is reacting

mol of C8H18 reacting = (2/16)* moles of CO2

= (2/16)*3.7878

= 0.4735 mol

Molar mass of C8H18 = 8*MM(C) + 18*MM(H)

= 8*12.01 + 18*1.008

= 114.224 g/mol

mass of C8H18 = number of mol * molar mass

= 0.4735*114.224

= 54.1 g

Answer: 54.1 g

11. Using the following equation for the combustion of octane,
calculate the amount of grams of carbon dioxide formed from 100.0 g
of octane. C8H18 + O2 → CO2 + H2O ΔH°rxn = -11018 kJ

1. The combustion of gasoline (C8H18) with
excess oxygen produces carbon dioxide and water.
-Write a balanced chemical reaction for the combustion of
gasoline to yield carbon dioxide and water.
-Presuming that a tank of gasoline contains 80 liters and that
its density is 0.77 kg/liter, determine how many kg of
CO2 are produced for each tank of gasoline burned.
Also, the products for octane + O2 should be carbon
dioxide and water. Now, you have to write it in...

Write the balanced equation for the combustion of isooctane
(C8H18) to produce carbon dioxide and water.
Use the smallest possible integers to balance the
equation. Also, separate the + sign with 1 space.
Remember that a combustion reaction requires oxygen.
Use the smallest whole number coefficients in
your balanced equation.
Write the reactants in the order isooctane then oxygen. Write
the products in the order carbon dioxide then water.
Assuming gasoline is 90.0% isooctane, with a density of 0.692
g/mL,...

The combustion of octane, C8H18, proceeds according to the
reaction shown. 2C8H18(l)+25O2(g)⟶16CO2(g)+18H2O(l) If 514 mol of
octane combusts, what volume of carbon dioxide is produced at 38.0
∘C and 0.995 atm?

Here is the combustion reaction for octane (C8H18), which is a
primary component of gasoline. How many moles of CO2 are emitted
into the atmosphere when 24.1 g of C8H18 is burned?

A 1.000 g sample of octane (C8H18) is burned in a bomb
calorimeter containing 1200 grams of water at an initial
temperature of 25.00ºC. After the reaction, the final temperature
of the water is 33.20ºC. The heat capacity of the calorimeter (also
known as the “calorimeter constant”) is 837 J/ºC. The specific heat
of water is 4.184 J/g ºC. Calculate the heat of combustion of
octane in kJ/mol.

The octane rating of gasoline is a relationship of the burning
efficiency of the given gasoline mixture to the burning efficiency
of octane (C8H18). Like most of hydrocarbons,
octane reacts with oxygen gas to produce carbon dioxide and water.
The unbalanced equation for this reaction:
C8H18 (l) + O2(g) → CO2
(g) + H2O (g)
If 0.240 mol of octane is allowed to
react with 0.890 mol of oxygen gas,
how many moles of water are produced in this...

Determine how many grams of CO2 are produced by burning 7.49 g
of C4H10. _____g carbon dioxide and Balance the chemical equation
for this combustion reaction.

Octane has a density of 0.692g/ml how many grams of O2 is needed
to burn down 17 gal of C8H18

Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to
produce gaseous carbon dioxide CO2 and gaseous water H2O . Suppose
8.00 g of octane is mixed with 39. g of oxygen. Calculate the
maximum mass of carbon dioxide that could be produced by the
chemical reaction. Round your answer to 3 significant digits.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 10 minutes ago

asked 16 minutes ago

asked 24 minutes ago

asked 25 minutes ago

asked 27 minutes ago

asked 28 minutes ago

asked 31 minutes ago

asked 32 minutes ago

asked 35 minutes ago

asked 35 minutes ago

asked 38 minutes ago

asked 39 minutes ago