Question

Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00 atm and 23 ∘C, what is the volume of carbon dioxide formed by the combustion of 1.60 g of butane?

Answer #1

Molar mass of C4H10 = 4*MM(C) + 10*MM(H)

= 4*12.01 + 10*1.008

= 58.12 g/mol

mass of C4H10 = 1.6 g

mol of C4H10 = (mass)/(molar mass)

= 1.6/58.12

= 0.0275 mol

From balanced chemical reaction, we see that

when 2 mol of C4H10 reacts, 8 mol of CO2 is formed

mol of CO2 formed = (8/2)* moles of C4H10

= (8/2)*0.0275

= 0.1101 mol

we have:

P = 1.0 atm

n = 0.1101 mol

T = 23.0 oC

= (23.0+273) K

= 296 K

we have below equation to be used:

P * V = n*R*T

1 atm * V = 0.1101 mol* 0.0821 atm.L/mol.K * 296 K

V = 2.68 L

Answer: 2.68 L

Butane, C4H10 , is a component of natural gas that is used as
fuel for cigarette lighters. The balanced equation of the complete
combustion of butane is
2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l)
At 1.00 atm and 23 ∘C , what is the volume of carbon dioxide
formed by the combustion of 1.60 g of butane?
Express your answer with the appropriate units.
volume of CO2 =

Butane, C4H10, is a component of natural gas that is used as
fuel for cigarette lighters. The balanced equation of the complete
combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.01
bar and 23 ∘C, what is the volume of carbon dioxide formed by the
combustion of 2.60 g of butane?

Butane, C4H10, is a component of natural gas that is used as
fuel for cigarette lighters. The balanced equation of the complete
combustion of butane is 2C4H10(g)+13O2(g)→8CO2(g)+10H2O(l) At 1.00
atm and 23 ∘C, what is the volume of carbon dioxide formed by the
combustion of 2.80 g of butane? what is the volume of CO2?The ideal
gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant R equals 0.08206...

The ideal gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant Requals 0.08206 L⋅atm/(K⋅mol) or 8.3145
J/(K⋅mol). The equation can be rearranged as follows to solve for
n:
n=PVRT
This equation is useful when dealing with gaseous reactions
because stoichiometric calculations involve mole ratios.
A)When heated, calcium carbonate decomposes to yield calcium
oxide and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)
What is the mass of calcium carbonate...

± Stoichiometric Relationships with Gases
The ideal gas law
PV=nRT
relates pressure P, volume V, temperature
T, and number of moles of a gas, n. The gas
constant Requals 0.08206 L⋅atm/(K⋅mol) or 8.3145
J/(K⋅mol). The equation can be rearranged as follows to solve for
n:
n=PVRT
This equation is useful when dealing with gaseous reactions because
stoichiometric calculations involve mole ratios.
Part A
When heated, calcium carbonate decomposes to yield calcium oxide
and carbon dioxide gas via the reaction
CaCO3(s)→CaO(s)+CO2(g)...

Butane C4H10 is a common fuel found in
cigarette lighters. When butane burns, it combines with oxygen to
produce carbon dioxide and water. A student burned a 5.00-gram
sample of butane. Show all calculations in solving the following
problems.
1. Write the balanced equation for the combustion of butane.
2. Find the number of moles of butane in 5.00 grams.
3. Find the number of moles of oxygen that will react with 5.00
g of butane.
4. Find the number...

1.) Imagine that you have a 7.00 L gas tank and a 4.00 L gas
tank. You need to fill one tank with oxygen and the other with
acetylene to use in conjunction with your welding torch. If you
fill the larger tank with oxygen to a pressure of 155 atm , to what
pressure should you fill the acetylene tank to ensure that you run
out of each gas at the same time? Assume ideal behavior for all
gases....

Butane, the fuel used in cigarette lighters, burns according to
the equation: 2 C4H10 (g) + 13 O2 (g) 8 CO2 (g) + 10 H2O(g) H =
– 5316 kJ a) Calculate the mass of oxygen that must react in order
for this reaction to generate 2150 kJ of heat b) Calculate the
amount of heat, including sign, that is transferred when 75.0 g of
butane react completely.

Mass C4H10
Mass O2
Mass CO2
Mass H2O
1.31 g
5.72g
11.12g
8.84g
222 mg
148mg
Consider the following balanced equation for the combustion of
butane, a fuel often used in lighters.
2C4H10(g)+13O2(g)?8CO2(g)+10H2O(g)
Complete the following table, showing the appropriate masses of
reactants and products. If the mass of a reactant is provided, fill
in the mass of other reactants required to completely react with
the given mass, as well as the mass of each product formed. If the
mass...

2C4H10(g)+13 O2(g)--> 10H2O(g)+8CO2(g)
A. calculate the mass of water produced when 6.30g of
butane (C4H10) reacts with excess oxygen.
B. calculate the mass of butane needed to produce
47.2g of carbon dioxide

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