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Lecture 6. 3.6: Quantitative Information from Balanced Equations.

Lecture 6. 3.6: Quantitative Information from Balanced Equations. 2 H 2 + (1) O 2 ? 2 H 2 O 2 moles 1 mole 2 moles. 3.6: Quantitative Information from Balanced Equations.

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HIGHER CHEMISTRY REVISION .

HIGHER CHEMISTRY REVISION. Unit 1:- The Mole. 1. The balanced equation for the decomposition of hydrogen peroxide into water and oxygen is: 2H 2 O 2 (l) ? 2H 2 O(l) + O 2 (g) . 24000 cm 3 of gas = 1 mol of O 2 So 40 cm 3 = 0.0167 mol

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Excess

Excess. mass n gfm. n C V (l). Calculate the number of moles of each reactant:- Number of moles in 10g of CaCO 3 = 10 / 100 = 0.1 Number of moles of HCl = 1 x 100 / 1000 = 0.1. HIGHER GRADE CHEMISTRY CALCULATIONS.

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HIGHER GRADE CHEMISTRY CALCULATIONS

mass n gfm. n C V (l). Calculate the number of moles of each reactant:- Number of moles in 10g of CaCO 3 = 10 / 100 = 0.1 Number of moles of HCl = 1 x 100 / 1000 = 0.1. HIGHER GRADE CHEMISTRY CALCULATIONS.

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Lecture 6. 3.6: Quantitative Information from Balanced Equations.

HIGHER CHEMISTRY REVISION .

Excess

HIGHER GRADE CHEMISTRY CALCULATIONS