Question

Stoichiometry (How are masses of reactants and products related?) Model 1: The Balanced Chemical Equation As we saw in ChemActivity 19. a balanced chemical reaction can be interpreted in two ways. First, it can describe how many molecules of reactants are consumed in order to produce a certain number of molecules of products. Second, it can describe how many moles of reactants are consumed in order to produce the indicated number of moles of products. | 3 H2 (9) + N2 (g) – 2 NH3 (g) (1) 2 CO (9) + O2 (9) 2002 (9) (2) Critical Thinking Questions: 1. How many NH, molecules are produced for every N, molecule that is consumed in reaction (1)? 2. How many moles of N2 react to produce 8 moles of NH, in reaction (1)? -_ mol N2 3. Discuss with your team, and describe in a sentence how you calculated the answer to CTQ 2. 4. Show your work for CTQ 2 as a unit conversion. Make sure that your conversion factor contains units. 5. How many moles of Co, will be formed when 0.25 mol of Oz react in reaction (2)? Show your work, including a conversion factor. 6. For reaction (2): a. What is the molar mass of Oz (grams per mole)? b. How many moles of O, will react when starting with 10.0 g of Oz? Show your work, with a conversion factor. C. How many moles of CO, will be produced when the moles of O, calculated in (b) are consumed? Show work. d. How many grams of CO2 will be produced from the moles of CO, calculated in (c)?

Answer 1

1) For every one molecule of N2, two molecules of NH3 produce.

2) 4 moles of N2 react to give 8 moles of NH3.

3) According to the balanced reaction,

2 mole NH3 require 1 mole N2

8 mole NH3 require 8/2 = 4 mole N2