Stochiometry

A limiting reactant is a reactant that.....

• runs out during a chemical reaction

• causes a reaction to stop

• determines the amount of products that can be made

• all of these

Tags

NGSS.HS-PS1-7

Using the following equation:

Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)

How many moles of iron can be made from 6 moles H₂ and excess Fe₂O₃?

• 4 moles Fe

• 6 moles Fe

• 9 moles Fe

• 2 moles Fe

Tags

NGSS.HS-PS1-7

The limiting reactant

• slows the reaction down

• is used up first

• is the reactant that is left over

• controls the speed of the reaction

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

• 1.16%

• 116%

• 85%

• 76%

Tags

NGSS.HS-PS1-7

The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting

• Percent

• actual

• stoichiometry

• theoretical

When reacting Na with Cl₂, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

• 90.4%

• 104%

• 96.15%

• 1.04%

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

• theoretical yield

• mole ratio

• actual yield

• percentage yield

What is the measured amount of a product obtained from a chemical reaction?

• mole ratio

• theoretical yield

• percentage yield

• actual yield

Tags

NGSS.HS-PS1-7

Mole ratios are obtained from the

• balanced chemical equation

• periodic table

• molar mass

What is the mole ratio of H₂O to H₃PO₄ in the following chemical equation?   P₄O₁₀ + 6 H₂O --> 4 H₃PO₄ 

• 6:4

• 4:6

• 1:3

• 3:1

Tags

NGSS.HS-PS1-7