Chemical Reactions Using Simple Stoichiometry Problems

What is the molar mass of CH₄

• 16.0
• 16.4
• 16.03
• 13

2H₂   +   O₂    −−〉 2H₂O
8.3 moles H₂ −−〉moles H₂O

• 4.15
• 8.3
• 16.6
• 74.04

Tags

NGSS.HS-PS1-7

2H₂  +   O₂    −−〉 2H₂O
3.91 g O₂ −−〉g H₂O

• 1.905
• 4.4
• 2.2
• 1.1

Tags

NGSS.HS-PS1-7

Find the percent yield
2Fe₂O₃   +   3C  −−〉  4Fe   +   3CO₂

Given 38.1 grams iron(III) oxide and 9.53 grams of carbon, find the percent yield if the actual yield is 17.41 grams of iron.

• 65.3
• 29.4
• 26.65
• 59.14

What is the molar mass of Ba(CN)₂

• 189.3
• 189.0
• 189
• 189.4

When 12 moles of O₂ reacts with 1.1 mole of C₁₀H₈ what is the limiting reactant?  C₁₀H₈ + 12 O₂ --> 10 CO₂ + 4 H₂O

• Oxygen
• C₁₀H₈
• Water
• Carbon Dioxide

Tags

NGSS.HS-PS1-7

In a lab, a scientist calculates he should produce 12.3 grams of product in his experiment. When he is finished collecting his product, it weighs 10.1 grams. What is his percent yield?

• 82%
• 0.82%
• 10.1 %
• 100%

Tags

NGSS.HS-PS1-7

Molar masses are determined from

• the mole ratio of a given amount of reactant to an unknown amount of product
• the periodic table
• any mole ratio in the equation
• a conversion factor

What is the mass of one mole of aluminum?

• 27 g
• 13 g
• 53.985 g
• 14 g

Actual yield must be determined by

• experiments
• calculations
• theoretical yield
• estimation