Question

Calculate the amount of water (g) produced by the combustion of 16 g of methane

Answer 1

Answer:

According to the above equation, one mole of CH4 (16 g) on combustion gives one mole of carbon dioxide and 2 moles of water and 2 moles of water = 2 x [2 + 16] = 36 g of water.

Answer 2

The mass of water produced by the reaction is 32 grams

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$     .....(1)

Given mass of methane = 16 g

Molar mass of methane = 16 g/mol

Putting values in equation 1, we get:

$\text{Moles of methane}=\frac{16g}{16g/mol}=1mol$

The chemical equation for the combustion of methane follows:

$CH_4+2O_2\rightarrow CO_2+2H_2O$

By Stoichiometry of the reaction:

1 mole of methane produces 2 moles of water

Now, calculating the mass of water from equation 1, we get:

Molar mass of water = 18 g/mol

Moles of water = 2 moles

Putting values in equation 1, we get:

$2mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(2mol\times 18g/mol)=32g$

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