Defining Stoichiometry

In the reaction: P₄ + 6Cl₂ ---> 4PCl₃, how many atoms of Chlorine are in the reactant?

• 1

• 2

• 6

• 12

Tags

NGSS.MS-PS1-5

In the reaction: P₄ + 6Cl₂ ---> 4PCl₃, how many molecules of Phosphorous Chloride are there in the product?

• 1

• 2

• 4

• 12

Tags

NGSS.HS-PS1-7

How many liters of NH₃ are needed to react completely with 30.0L of NO?
4NH₃+6NO --> 5N₂ + 6H₂O

• 5.0 L

• 20.0 L

• 7.5 L

• 120.0 L

Tags

NGSS.HS-PS1-7

Cl₂ + 2KBr → Br₂ + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?

• 749 g

• 223 g

• 479 g

• 814 g

Tags

NGSS.HS-PS1-7

What is stoichiometry?

• The study of the speed of chemical reactions

• The calculation of reactants and products in chemical reactions

• The study of energy changes in chemical reactions

• The study of chemical bonds

Tags

NGSS.HS-PS1-7

In the reaction @@ ext{2H}_2 + ext{O}_2 ightarrow ext{2H}_2 ext{O}@@, how many moles of water are produced from 4 moles of hydrogen gas?

• 1 mole

• 2 moles

• 4 moles

• 8 moles

Tags

NGSS.HS-PS1-7

Which of the following best describes the law of conservation of mass in stoichiometry?

• Mass is created during a chemical reaction

• Mass is destroyed during a chemical reaction

• Mass is conserved and remains constant during a chemical reaction

• Mass is irrelevant in chemical reactions

Tags

NGSS.HS-PS1-7

If 5 moles of nitrogen gas react with hydrogen gas to form ammonia according to the equation @@ ext{N}_2 + 3 ext{H}_2 ightarrow 2 ext{NH}_3@@, how many moles of ammonia are produced?

• 5 moles

• 10 moles

• 15 moles

• 20 moles

Tags

NGSS.HS-PS1-7

In a stoichiometric calculation, what is the purpose of using a balanced chemical equation?

• To determine the speed of the reaction

• To identify the limiting reactant

• To ensure the correct proportions of reactants and products

• To measure the temperature change

Tags

NGSS.HS-PS1-7

How many grams of water are produced when 2 moles of hydrogen gas react with excess oxygen gas? (Molar mass of water = 18 g/mol)

• 18 grams

• 36 grams

• 54 grams

• 72 grams