Question

If 2.50 × 2 of the fifth grams of methane is combusted how many grams of water will be produced

Answer 1

[AI-generated answer — Bot GPT 3.5]

The chemical equation for the combustion of methane is:

CH4 + 2O2 -> CO2 + 2H2O

From the equation, it can be seen that for every mole of methane (CH4) that is combusted, 2 moles of water (H2O) are produced.

To calculate the amount of water produced when 2.50 grams of methane is combusted, we first need to convert the mass of methane to moles:

Molar mass of CH4 = 12.01 + 4*(1.008) = 16.05 g/mol

Number of moles of CH4 = 2.50 g / 16.05 g/mol = 0.156 moles

Since 1 mole of CH4 produces 2 moles of H2O, we can calculate the amount of water produced:

Number of moles of H2O = 0.156 mol x 2 = 0.312 mol

Now, we convert moles of water to grams:

Molar mass of H2O = 2*(1.008) + 15.999 = 18.02 g/mol

Mass of water produced = 0.312 mol x 18.02 g/mol = 5.62 grams

Therefore, if 2.50 grams of methane is combusted, 5.62 grams of water will be produced.