Question

Methane and oxygen react to form carbon dioxide and water. what mass of water is formed if 0.80 g of methane reacts with 3.2 g of oxygen to produce 2.2 g of carbon dioxide?

Answer 1

The Balance Chemical Equation is as follow,

                                CH₄  + 2 O₂   →   CO₂  +  2 H₂O

As 1 mole of CH₄ is equal to 16 g, then 0.8 g is equal to 0.05 moles.
Also, if 2 moles of O₂ is equal to 64 g, then 3.2 g is equal to 0.1 moles.
Now, moles of CO₂ and H₂O can also be calculated from equation. 
So, reacting 0.05 moles of CO₂ and 0.1 moles of O₂ will produce 0.05 moles (2.2 g) of CO₂ and 0.1 moles ( unknown mass) of H₂O)

Calculating for mass of H₂O,
As,
                             2 moles of H₂O is equal to   =   36 g of H₂O
Then
                   0.1 moles of H₂O will be equal to   =   X g of H₂O

Solving for X,
                                      X  =  (0.1 mol × 36 g) ÷ 2 mol

                                      X  =  1.8 g of H₂O is produced

Answer 2

1.8 g

Further explanation

Given:

0.80 g of methane reacts with 3.2 g of oxygen to produce 2.2 g of carbon dioxide.

Question:

What mass of water is formed?

The Process:

Methane and oxygen react to form carbon dioxide and water. Remember this, the chemical activity that uses oxygen to produce light and heat is also called the combustion process.

In any chemical reaction, the sum of the masses of the reactants is equal to the sum of the masses of the products. That's right, this is called conservation of the masses.

Let us write the word equation of the chemical reaction and then solve the problem following the law of the conservation of mass.

$\boxed{ \ Methane + Oxygen \rightarrow Carbon \ dioxide + Water\ }$

$\boxed{ \ 0.80 \ g \ + \ 3.2 \ g \rightarrow 2.2 \ g \ + \ m_{Water}? \ }$

$\boxed{ \ m_{reactants} = m_{products} \ }$

$\boxed{ \ 0.80 \ g \ + \ 3.2 \ g = 2.2 \ g \ + \ m_{Water} \ }$

Rewrite by rearranging as follows:

$\boxed{ \ 2.2 \ g \ + \ m_{Water} = 0.80 \ g \ + \ 3.2 \ g \ }$

$\boxed{ \ 2.2 \ g \ + \ m_{Water} = 4.0 \ g \ }$

$\boxed{ \ m_{Water} = 4.0 \ g - 2.2 \ g \ }$

Thus the mass of water formed is 1.8 g.

The balanced equation with state symbols is:

$\boxed{ \ CH_4_{(g)} + 2O_2_{(g)} \rightarrow CO_2_{(g)} + 2H_2O_{(l)} \ }$

Notes:

• The French scientist Antoine Laurent Lavoisier represented his essential contribution by declaring the law of conservation of mass as one of the fundamental laws in chemistry.
• The law of the conservation of the mass states that in a chemical reaction the sum of the masses of the reactants is equal to the sum of the masses of the products. $\boxed{\boxed{ \ m_{reactants} = m_{products} \ }}$

Learn more

1. Flammability as one of the chemical properties brainly.com/question/1767022
2. Carbon atoms can form four covalent bonds brainly.com/question/3064597
3. About the solution as a homogeneous mixture  brainly.com/question/637791

Keywords: methane and oxygen, react to form carbon dioxide and water, combustion, to produce, the conservation of mass, the word equation, the balanced equation, Lavoisier