Download presentation

Presentation is loading. Please wait.

Published bySavannah Greeney Modified about 1 year ago

1
SECTION 9.1 The Arithmetic of Equations

2
Interpreting Chemical Equations In terms of moles: Example Equation: 2H 2 + O 2 2H 2 O 2 mol H2 +1 mol O2 =2 mol H2O

3
Interpreting Chemical Equations In terms of particles: You know that Avogradro’s Number relates particles and moles (6.02 x particles = 1 mole) Example Equation: 2H 2 + O 2 2H 2 O 2 mol H2 x 6.02 x particles + 1 mol 1 mol O2 x 6.02 x particles = 1 mol 2 mol H2 x 6.02 x particles 1 mol x particles of H x particles of O2 =1.204 x particles of H2O

4
Interpreting Chemical Equations In terms of mass: 1 mole = molar mass of element or compound Example Equation: 2H 2 + O 2 2H 2 O 2 mol H2 x grams + 1 mol 1 mol O2 x grams = 1 mol 2 mol H2 x grams 1 mol grams of H grams of O2 = grams of H2O

5
Interpreting Chemical Equations In terms of volume: 1 mole = 22.4 Liters Example Equation: 2H 2 + O 2 2H 2 O 2 mol H2 x 22.4 L + 1 mol 1 mol O2 x 22.4 L = 1 mol 2 mol H2 x 22.4 L 1 mol 44.8 L of H L of O2 =44.8 L of H2O

6
After reading Section 9.1, you should know: How to balance a chemical equation How to calculate particles, moles, volume and mass from a balanced equation

Similar presentations

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google