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Mole Ratios, Slides of Chemistry

Facultés Universitaires Catholiques de MonsChemistry

b. Use mathematical concepts to explain how your answer in part a is possible. 6. The ratio obtained from the coefficients in a balanced chemical equation is ...

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Mole Ratios 1
Mole Ratios
How can the coefficients in a chemical equation be interpreted?
Why?
A balanced chemical equation can tell us the number of reactant and product particles (ions, atoms,
molecules or formula units) that are necessary to conserve mass during a chemical reaction. Typically
when we balance the chemical equation we think in terms of individual particles. However, in real life
the reaction represented by an equation occurs an unimaginable number of times. Short of writing very
large numbers (1023 or larger) in front of each chemical in the equation, how can we interpret chemical
equations so that they more realistically represent what is happening in real life? In this activity you will
explore the different ways a chemical reaction can be interpreted.
Model 1 – A Chemical Reaction
N2(g) + 3H2(g) → 2NH3(g)
1. Consider the reaction in Model 1.
a. What are the coefficients for each of the following substances in the reaction?
N2 H2 NH3
b. Draw particle models below to illustrate the reaction in Model 1.
2. Consider each situation below as it relates to the reaction in Model 1.
a. Calculate the amount of reactants consumed and products made.
b. Record the ratio of N2 to H2 to NH3. Reduce the ratio to the lowest whole numbers possible.
N2
Consumed
H2
Consumed
NH3
Produced
Ratio N2:H2:NH3
(reduced)
For a single reaction, how many
molecules of each substance would
be consumed or produced?
If the reaction occurred one hun-
dred times, how many molecules
would be consumed or produced?
If the reaction occurred 538 times,
how many molecules would be
consumed or produced?
pf3
pf4
pf5

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Mole Ratios 1

Mole Ratios

How can the coefficients in a chemical equation be interpreted?

Why?

A balanced chemical equation can tell us the number of reactant and product particles (ions, atoms, molecules or formula units) that are necessary to conserve mass during a chemical reaction. Typically when we balance the chemical equation we think in terms of individual particles. However, in real life the reaction represented by an equation occurs an unimaginable number of times. Short of writing very large numbers (10^23 or larger) in front of each chemical in the equation, how can we interpret chemical equations so that they more realistically represent what is happening in real life? In this activity you will explore the different ways a chemical reaction can be interpreted.

Model 1 – A Chemical Reaction

N 2 (g) + 3H 2 (g) → 2NH 3 (g)

  1. Consider the reaction in Model 1. a. What are the coefficients for each of the following substances in the reaction? N 2 H 2 NH 3 b. Draw particle models below to illustrate the reaction in Model 1.
  2. Consider each situation below as it relates to the reaction in Model 1. a. Calculate the amount of reactants consumed and products made. b. Record the ratio of N 2 to H 2 to NH 3. Reduce the ratio to the lowest whole numbers possible. N 2 Consumed

H 2

Consumed

NH 3

Produced Ratio N 2 :H 2 :NH 3 (reduced) For a single reaction, how many molecules of each substance would be consumed or produced? If the reaction occurred one hun dred times, how many molecules would be consumed or produced? If the reaction occurred 538 times, how many molecules would be consumed or produced?

2 POGIL™^ Activities for High School Chemistry

  1. Refer to the data table in Question 2. a. How do the reduced ratios in the last column compare to the coefficients in the reaction shown in Model 1? b. Use mathematical concepts to explain how your answer in part a is possible.
  2. Even 538 is a small number of molecules to use in a reaction. Typically chemists use much larger numbers of molecules. (Recall that one mole is equal to 6.02 x 10^23 particles.) Consider each situation below as it relates to the reaction in Model 1: N 2 (g) + 3H 2 (g) → 2NH 3 (g). a. Calculate the amount of reactants consumed and products made. b. Record the ratio of N 2 to H 2 to NH 3. Reduce the ratio to the lowest whole number possible. N 2 Consumed

H 2

Consumed

NH 3

Produced Ratio N 2 :H 2 :NH 3 If the reaction occurred 6.02 × 1023 times, how many molecules would be consumed or pro duced? How many moles of each sub stance would be consumed or produced in the previous situa tion?

  1. Refer to the data table in Question 4. a. How do the reduced ratios in the last column compare to the coefficients in the reaction in Model 1? b. Use mathematical concepts to explain how your answer in part a is possible.
  2. The ratio obtained from the coefficients in a balanced chemical equation is called the mole ratio. a. What is the mole ratio for the reaction in Model 1? b. Explain why this ratio is called the mole ratio?

4 POGIL™^ Activities for High School Chemistry

Model 2 – Proposed Calculations for Mass of NH 3 to Mass of N 2

Toby’s Method x grams 1 mole N 2 ———— = ————— ➞ x = ______ g N 2 30.0 g 2 moles NH 3 Rachel’s Method 1 mole NH 3 30.0 g NH 3 × ————— = ______ moles NH 3 17.0 g NH 3 x mole N 2 1 mole N 2 —–————– = ————— ➞ x = ______ moles N 2 _____ mole NH 3 2 moles NH 3 28.0 g N 2 ______ mole N 2 × ———— = ______ g N 2 1 mole N 2 Jerry’s Method 1 mole NH 3 1 mole N 2 28.0 g N 2 30.0 g NH 3 × ————— × ————— × ———— = ______ g N 2 17.0 g NH 3 2 moles NH 3 1 mole N 2

  1. Model 2 shows three proposed calculations to solve the problem in Question 10. Complete the calculations in Model 2 by filling in the underlined values.
  2. Which method does not use the mole ratio in an appropriate manner? Explain.
  3. Two of the methods in Model 2 give the same answer. Show that they are mathematically equivalent methods.
  4. Use either Rachel or Jerry’s method from Model 2 to calculate the mass of hydrogen needed to make 30.0 g of ammonia. N 2 (g) + 3H 2 (g) → 2NH 3 (g)

Mole Ratios 5

Extension Questions

  1. One mole of any gas will occupy 22.4 L of volume at standard temperature and pressure (STP). Consider this situation as it relates to the reaction in Model 1: N 2 (g) + 3H 2 (g) → 2NH 3 (g) a. Calculate the volumes of reactants consumed and the volume of product made. b. Record the ratio of N 2 to H 2 to NH 3. Reduce the ratio to the lowest whole numbers possible. N 2 Consumed

H 2

Consumed

NH 3

Produced Volume Ratio N 2 :H 2 :NH 3 How many liters of each sub stance would be consumed or produced if the reaction occurred 6.02 × 10^23 times at STP?

  1. Refer to the data table in Question 15. a. Can the mole ratio from a balanced chemical equation be interpreted as a ratio of volumes for gases? b. Use mathematical concepts to explain how your answer in part a is possible.
  2. Explain why the ratio of volumes is NOT followed in the following reactions. 2H 2 (g) + O 2 (g) → 2H 2 O(l) NH 3 (g) + HCl(g) → NH 4 Cl(s) 44.8 L 22.4 L 0.036 L 22.4 L 22.4 L 0.035 L
  3. Which of the following quantities are conserved (total amount in reactants = total amount in products) in a chemical reaction? Find an example or counter example from this activity to sup port your answer for each. a. Molecules b. Moles c. Mass d. Volume e. Atoms of an element