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Moles and equations. Chapter 1: Moles and equations. 1. Learning outcomes. you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12C scale. empirical formula and molecular formula. the mole in terms of the Avogadro constant.
Use the formula below to answer questions 1- 4 3Cu + 8HNO 3 3Cu(NO 3) 2 + 2NO + 4H 2 O 1. What is the mole ratio of copper to nitrogen monoxide in this reaction? 2. If 1.50 moles of copper are used, how many moles of NO are produced? 3. If 4.50 moles of HNO 3 are used, how many moles of copper (II) nitrate are produced? 4.
EXAMPLE 1: How many moles are in 39.0 grams of LiF? EXAMPLE 2: What is the number of moles of potassium chloride present in 148 g? How to Convert from Moles to Grams:
Mole Calculations Answers. 1a. Mr of CH3OH = 12.0 + (3 x 1.01) + 16.0 + 1.01 = 32.0 g mol–1. 1b. Moles CH3OH = mass / Mr = 5.0 / 32.0 = 0.16 mol. (Answer to 2 significant figures as mass given to 2 significant figures.) 2. Mr of CO2 = 12.0 + (16.0 x 2) = 44.0 g mol–1 Mass of CO2 = Mr x moles = 44.0 g x 0.50 g mol–1 = 22 g . 3a.
Mole Calculation Practice Worksheet Answer the following questions: 1) How many moles are in 25.0 grams of water? 2) How many grams are in 4.500 moles of Li 2O? 3) How many molecules are in 23.0 moles of oxygen? 4) How many moles are in 3.4 x 10 23 molecules of H 2SO 4? 5) How many molecules are in 25.0 grams of NH 3?
Chapter 1. Moles and equations. Chapter outline. Relative atomic mass, isotopic mass and formula mass based on the 12C scale. Empirical formula and molecular formula. Using mass spectra to calculate relative atomic mass. Constructing balanced equations. Performing calculations involving moles, reacting masses, gas volumes and solution concentration
1) A mole of anything is how many? (give the number): 2) Why is it that different amounts of things can still equal one mole? (think about the weight of a dozen elephants vs a dozen eggs) 3) Why do we want to use the concept of moles?
