What mass of water is produced from the complete combustion of 7.30 10−3 g of methane

2016-09-15T18:03:15-04:00

What mass of water is produced from the complete combustion of 4.00×10−3 g of methane?

2016-09-17T09:01:13-0400

Methane combustion follows the equation CH4 + 2O2 = CO2 + 2H2O. Thus, 4.00*10-3 g of methane is 4.00*10-3 g/16 g/mol = 2.5*10-4 mol and it produces 5*10-4 mol of water or 5*10-4 mol * 18 g/mol = 9*10-3 g of it.

1 Expert Answer

Nathan I. answered • 04/23/19

Patient, Knowledgeable Tutor in Chemistry

First, we need to balance the stoichiometry equation.

?CH4(g) + ?O2(g) --> ?CO2(g) + ?H2O(g)

Lets start by putting 1 for each question mark. There are 2 hydrogens in water, and 4 in methane. This means whatever number we put in front of methane, the number in front of H2O has to be double that. If we put a 2 in front of H2O, the only thing unbalanced in the equation in the number of oxygens: there are four on the right side and only two in the oxygen on the left. We can make the coefficient in front of oxygen 2:

1CH4(g) + 2O2(g) --> 1CO2(g) + 2H2O(g)

But, to use the stoichiometry equation, we need to figure out the number of moles of methane used, instead of grams. The molecular weight of methane is 16.043g/mol. We can use this to find the moles of methane:

1.2*10^-3g / (16.043g/mol)=7.48*10^-5 moles of methane

Now that we know the number of moles of methane combusted, we can use the stoichiometry equation to find out how many moles of CO2 this equates to. For every mole of methane burned, a mole of CO2 is produced:

7.48*10^-5 mol CH4 * (1 mol CO2 / 1 mol CH4) = 7.48*10^-5 mol CO2

We know that the reaction goes to completion, so all the methane will be reacted. To find the mass of carbon dioxide used, we can use the number of moles from the above equation, and the molecular weight of CO2 (= 44.009 g/mol).

7.48*10^-5 mol CO2 * 44.009 g/mol = 3.29*10^-3 g CO2

The mass of CO2 produced is 3.29*10^-3g.

1 Expert Answer

The mass of water produced from the complete combustion of 4.20 x 10-3 g CH4 is 9.43 x 10-3 g H2O.

What is the amount of water produced by the complete combustion of 16 g of methane?

36 g
Since, the given weight of methane is 16 g, hence the water produced by the combustion of 16 g of methane is 36 g.

How do you find the mass of H2O produced by combustion?

Mass of 0.5 mol H2O = 9.0g ( answer to 2 significant digits.) So1 mole of methane on complete combustion gives = 2 moles =36 gm of water. 0.25 mole of methane on complete combustion gives= 36 x 0.25=9.00 gm.

What amount of water is produced by combustion of 32g of methane?

Answer: 72 grams of water will be produced.

How much co2 is produced from natural gas?

Pounds of CO2 emitted per million British thermal units (Btu) of energy for various fuels

Explanation: 1 mol of methane is 16 grams. Therefore, if you have 100 grams of methane, it means that you have 10016=6.25 moles of methane. When you burn 6.25 moles of methane, you produce 6.25 moles of carbondioxide.

What is combustion of methane?

The combustion of methane means that it is possible to burn it. Chemically, this combustion process consists of a reaction between methane and oxygen in the air. When this reaction takes place, the result is carbon dioxide (CO2), water (H2O), and a great deal of energy.

What is the mass of water produced?

You first need to determine the number of moles of water produced, then multiply the moles of water produced by its molar mass, 18.105 g/mol .

What does methane consist of?

Methane is the simplest hydrocarbon, consisting of one carbon atom and four hydrogen atoms. Methane is a powerful greenhouse gas. Although the concentration of methane in Earth’s atmosphere is small (around 1.8 parts per million), it is an important greenhouse gas because it is such a potent heat absorber.

Is natural gas a clean energy?

Natural gas is a relatively clean burning fossil fuel Burning natural gas for energy results in fewer emissions of nearly all types of air pollutants and carbon dioxide (CO2) than burning coal or petroleum products to produce an equal amount of energy.

What is the maximum mass of methane CH4 that can be burned if only 1.0 g of oxygen is available?

So, our answer is . 5g.

What is the charge of methane?

Each hydrogen is assigned one of the two electrons it shares with the central carbon atom; the formal charge on each hydrogen atom in methane is zero. The central carbon is assigned one of the two electrons it shares with each of the four hydrogens.

What mass of water will be produced from 2.70 moles Ca Oh 2?

Hence, 97.2 g of water will be produced from 2.70 moles of Ca(OH)2 reacting with HCl.

What is the mass of water produced from 445g of C57H110O6?

For the following reaction, the mass of water produced from 445 g of C57H110O6 is: 2C57H110O6(s) + 163O2(g) →114CO2(g) + 110 H2O(l)

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