Question

From the following balanced equation, CH, (g) +20,(9) + CO2(g) + 2 H2O(g) how many grams of H, O can be formed from 1.25 g CH ? • Your answer should have three significant figures.

Answer 1

Answer:

Explanation:

A mole ratio is ​the ratio between the amounts in moles of any two compounds involved in a chemical reaction. The mole ratio can be determined by examining the coefficients in front of formulas in a balanced chemical equation.

Step 1: write the balanced chemical equation.

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

Step 2: calculate the moles of CH₄

Moles of CH₄ = mass given / molar mass = ( 1.25 g / 16.04 g/mol ) = 0.078 mol

Step 3: Calculate the moles of H₂O can be formed

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

According to the reaction:
1 mol of CH₄ produce 2 mol of H₂O
so, 0.078 mol of CH₄ will produce=( 2 mol of H₂O  / 1 mol of CH₄ )× 0.078 mol of CH₄ = 0.156 mol of H₂O

Step 4: Calculation of mass of H₂O can be produced

we get moles of H₂O that can be produced = 0.156 mol

Mass of H₂O can be produced = ( moles ×molar mass ) = ( 0.156 mol × 18.01528 g/mol ) = 2.81 g