CHM101 Chapter 6 Lecture Quiz Part 1

Consider the following balanced equation for the reaction of iron and oxygen: 4Fe(s) + 3O2(g) → 2Fe2O3(s) Calculate the number of moles of O2(g) required to react with 0.80 mol Fe(s).

0.60 mol

Use the balanced equation given to determine the number of moles of O2 needed to react with 0.30 moles of C3H8. C3H8(g) + 5O2(g) → 3CO2(g)+ 4H2O(g)

1.5 mol

When 0.10 mol Al(s) is mixed with 0.10 mol O2(g), the following reaction occurs: 4Al(s) + 3O2(g) → 2Al2O3(s). Which of the following best describes what should happen?

All of the Al should react, and 0.050 mol Al2O3 should be produced.

Which of the following best shows the series of conversion steps for calculating the mass of MgO(s) that should be produced when 0.10 g Mg(s) reacts by the following reaction? 2Mg(s) + O2(g) → 2MgO(s)

Grams Mg -> Moles Mg -> Moles MgO -> Grams MgO

What quantity do you use to calculate the amount of product that should form in a reaction?

the amount of limiting reactant

What is the theoretical yield in a percent yield calculation?

the amount of product that should form, calculated from the limiting reactant