1answer.
Ask question
Login Signup
Ask question
All categories
  • English
  • Mathematics
  • Social Studies
  • Business
  • History
  • Health
  • Geography
  • Biology
  • Physics
  • Chemistry
  • Computers and Technology
  • Arts
  • World Languages
  • Spanish
  • French
  • German
  • Advanced Placement (AP)
  • SAT
  • Medicine
  • Law
  • Engineering
natka813 [3]
3 years ago
6

What mass of butane in grams is necessary to produce 1.5×103 kj of heat what mass of co2 is produced?

Chemistry
2 answers:
Alexandra [31]3 years ago
5 0

\boxed{32.7{\text{3 g}}} of butane is necessary to produce 1.5 \times {10^3}\;{\text{kJ}}of heat and \boxed{99.32\;{\text{g}}} of {\text{C}}{{\text{O}}_{\text{2}}} is produced.

Further explanation:

Stoichiometry:

It is used to determine the amount of species present in the reaction by the relationship between reactants and products. It is used to determine the moles of a chemical species when moles of other chemical species present in the reaction is given.

Consider the general reaction,

{\text{A}} + 2{\text{B}} \to 3{\text{C}}

Here,

A and B are reactants.

C is the product.

One mole of A reacts with two moles of B to produce three moles of C. The stoichiometric ratio between A and B is 1:2, the stoichiometric ratio between A and C is 1:3 and the stoichiometric ratio between B and C is 2:3.

Combustion reaction:

It is the reaction in which the reactant reacts with molecular oxygen to form carbon dioxide and a water molecule. Molecular oxygen acts as the oxidizing agent in these reactions. A large amount of heat is released and therefore combustion reactions are exothermic in nature.

The combustion of butane occurs as follows:

{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}+\frac{{13}}{2}{{\text{O}}_2} \to 4{\text{C}}{{\text{O}}_2} + 5{{\text{H}}_{\text{2}}}{\text{O}}

The value of \Delta {{\text{H}}_{{\text{reaction}}}} is -2658 kJ/mol. This indicates the heat produced when one mole of butane is combusted.

The number of moles of butane \left( {{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}} \right) required in the given reaction is calculated as follows:

\begin{aligned}{\text{Moles of }}{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}&=\left({-150{\text{0 kJ}}} \right)\left( {\frac{{{\text{1 mol}}}}{{ - 265{\text{8 kJ}}}}}\right)\\&=0.56{\text{43 mol}} \\ \end{aligned}

The formula to calculate the mass of butane \left({{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}}\right) is as follows:

{\text{Mass of }}{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}=\left( {{\text{Moles of }}{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}}\right)\left({{\text{Molar mass of }}{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}}\right)                   ...... (1)

The number of moles of {{\text{C}}_4}{{\text{H}}_{10}} is 0.5643 mol.

The molar mass of {{\text{C}}_4}{{\text{H}}_{10}} is 58 g/mol.

Substitute these values in equation (1).

\begin{aligned}{\text{Mass of }}{{\text{C}}_{\text{4}}}{{\text{H}}_{{\text{10}}}}&=\left( {{\text{0}}{\text{.5643 mol}}}\right)\left( {\frac{{{\text{58 g}}}}{{{\text{1 mol}}}}}\right)\\&=32.72{\text{94 g}}\\&\approx{\text{32}}{\text{.73 g}} \\ \end{aligned}

Therefore the mass of butane required is 32.73 g.

According to the reaction stoichiometry, one mole of {{\text{C}}_4}{{\text{H}}_{10}} produces four moles of {\text{C}}{{\text{O}}_{\text{2}}}. The moles of {\text{C}}{{\text{O}}_{\text{2}}} produced in the given reaction are calculated as follows:

\begin{aligned}{\text{Moles of C}}{{\text{O}}_{\text{2}}}&=\left({{\text{0}}{\text{.5643 mol }}{{\text{C}}_4}{{\text{H}}_{10}}}\right)\left({\frac{{{\text{4 mol C}}{{\text{O}}_{\text{2}}}}}{{1\;{\text{mol }}{{\text{C}}_4}{{\text{H}}_{10}}}}} \right)\\&=2.257{\text{2 mol}}\\\end{gathered}

The formula to calculate the mass of {\text{C}}{{\text{O}}_{\text{2}}} is as follows:

{\text{Mass of C}}{{\text{O}}_{\text{2}}} = \left( {{\text{Moles of C}}{{\text{O}}_{\text{2}}}} \right)\left( {{\text{Molar mass of C}}{{\text{O}}_{\text{2}}}} \right)              ...... (2)

Substitute 2.2572 mol for the moles of {\text{C}}{{\text{O}}_{\text{2}}} and 44 g/mol for the molar mass of {\text{C}}{{\text{O}}_{\text{2}}} in equation (2).

\begin{aligned}{\text{Mass of C}}{{\text{O}}_{\text{2}}}&=\left({{\text{2}}{\text{.2572 mol}}} \right)\left( {\frac{{{\text{44 g}}}}{{{\text{1 mol}}}}} \right)\\&=99.316{\text{8 g}}\\&\approx {\text{99}}{\text{.32 g}} \\ \end{aligned}

Therefore the mass of carbon dioxide produced is 99.32 g.

Learn more:

1. Calculate \Delta {\text{H}} for the reaction using Hess law: brainly.com/question/11293201

2. Calculate the hydroxide ion concentration: brainly.com/question/11293214

Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Mole concept

Keywords: butane, mass, CO2, C4H10, molar mass of CO2, molar mass of C4H10, 32.73 g, 99.32 g, 44 g/mol, 58 g/mol, moles of CO2, moles of C4H10, 2.2572 mol, 0.5643 mol, stoichiometry, one mole, four moles.

kari74 [83]3 years ago
4 0
The heat of reaction (i.e. combustion) of butane (C_{4} H_{10}) when reacted with oxygen (O_{2})  is -2658 kJ/mol butane, and the chemical reaction is given by: 

C_{4} H_{10} + \frac{13}{2} O_{2} ---> 4 CO_{2}  + 5 H_{2}O

The mass of butane required in the reaction is based on the heat produced by the reaction, which is given to be -1,500 kJ. The minus sign is added because the reaction releases heat (exothermic), which means that the products are in a "lower energy state" than the reactants. 

Dividing this with the heat of reaction per mole of butane reacted would give the number of moles butane required. Then, multiplying the answer with the molar mass of butane which is 58 grams/mole, will give the mass of butane required. 

Moles of butane = [(-1,500 kJ)/(-2658 kJ/mol butane)]
Moles of butane = 0.5643 moles butane

Mass of butane  = 0.5643 moles butane * 58 grams/mol butane
Mass of butane  = 32.73 grams butane

The mass of carbon dioxide (CO_{2}) can be determined by multiplying the moles of butane (C_{4} H_{10}) with the mole ratio of (CO_{2}) produced to the (C_{4} H_{10}) reacted, and then with the molar mass of (CO_{2}), which is 44 grams/mole. 

Mass of carbon dioxide produced 
    = 0.5643 moles butane * [4 moles CO_{2}/ 1 mole C_{4} H_{10}] * 44 grams/mole CO_{2}

Mass of carbon dioxide produced  
    = 99.32 grams CO_{2}

Thus, the mass of butane required is 32.73 grams, and the mass of carbon dioxide produced from the reaction of this amount of butane is 99.32 grams. 
                
You might be interested in
Can you test a hypothesis that hummingbirds spend most of their waking hours feeding
Vitek1552 [10]
Yes you can. in order to do this however, you would need to observe the hummingbird and study it closely
6 0
3 years ago
Which of the following accurately describes semiconductor diodes? A. Unlike junction diodes, point-contact diodes are enclosed i
Anna007 [38]
The correct answer is letter A: <span>Unlike junction diodes, point-contact diodes are enclosed in a suitable casing and have terminals for connecting them to a circuit.</span>
5 0
3 years ago
Read 2 more answers
Jack lives in a small city in the Pacific Northwest, where the temperatures are cool all year and the sky is frequently cloudy a
kirill [66]

Answer:

Preocouparcor   ,imsm oilp

Explanation:

3 0
3 years ago
What are the three physical properties of gases
daser333 [38]
They are described through the use of four physical properties or macroscopic characteristics: pressure, volume, number of particles (chemists group them by moles) and temperature.
5 0
3 years ago
Read 2 more answers
What mass of potassium iodide is needed to prepare 5.60 L of a 1.13 M solution
MrMuchimi
Given that the question gives us concentration (M) and volume, we can use these so get moles. remember that Molarity (M)= mol/ Liters, so if we want the moles, then

moles= M x L

moles= 1.13 x 5.60= 6.33 moles KI

now to get the mass in grams, we need the molar mass of potassium iodide (KI) which can be determined using the periodic table and add the masses of each atom.

molar mass KI= 39.1 + 127= 166.1 g/mol

6.33 mol (166 g/ 1 mol)= 1050 grams KI


8 0
3 years ago
Other questions:
  • What is the concentration of a 0.750 l solution that contains 52.0 g of glucose (c6h12o6)?
    7·1 answer
  • Which is larger an atom or a molecule? Explain your answer.
    7·1 answer
  • Is the sun 240,000 miles from earth?
    7·1 answer
  • Through the complete electrolysis of a sample of pure water, a student collects 14.0 grams of hydrogen gas and 112.0 grams of ox
    12·1 answer
  • There are two jars A and B containing food materials. Food in jar 'A' is picked with acetic acid while 'B' is not. food of which
    7·1 answer
  • What causes continental drift?
    15·2 answers
  • What is the pressure of 0.540 mol of an ideal gas at 35.5 L and 223 K? Use mc031-1.jpg and mc031-2.jpg.
    12·2 answers
  • If the half-life of 37Rb is 4.7x101 years, how long would it take for 0.5 grams of a 2 gram sample to radioactively decay?
    13·1 answer
  • For a constant waves speed,wavelength,of the wave increases with a(n)______
    12·1 answer
  • Does the following compound contain a polyatomic ion? CuCl2 *<br> Yes<br> No
    14·1 answer
Add answer
Login
Not registered? Fast signup
Signup
Login Signup
Ask question!