Stoichiometric Ratios

STP stands for

• Standard Temperature and Pressure

• Standard Temperature or Pressure

• Satisfied Temperature and Pressure

• Selected Temperature and Pressure

For the following balanced chemical equation

2K + F₂ --> 2KF

how many moles of KF are present?

• 2 mol of KF

• 1 mol KF

Tags

NGSS.HS-PS1-7

Using the balanced equation below

2Ca + O₂ --> 2CaO

Predict the number of particles of Ca

• 6.02x10²³

• 1.204x10²⁴

• 6.02x10²²

• 1.204x10²³

Tags

NGSS.HS-PS1-7

For the balanced equation shown below

4Fe + 3O₂ --> 2Fe₂O₃

What is the volume of O₂ gas at STP

• 22.4L

• 44.8L

• 67.2L

• 134.4L

Tags

NGSS.HS-PS1-7

6.0 mol of aluminium reacts with oxygen to form aluminium oxide. What is the amount of oxygen, in mol, needed for complete reaction?

4Al(s) + 3O₂(g) → 2Al₂O₃(s)

• 1.5

• 3.0

• 4.5

• 6.0

Tags

NGSS.HS-PS1-7

Nitrogen reacts with hydrogen to give ammonia, NH₃ in a closed container. How many moles of H₂ are needed to produce 25 mol of NH₃?

N₂ + 3H₂ → 2NH₃

• A) 12.5

• B) 25

• C) 37.5

• D) 50

• E) 62.5

Tags

NGSS.HS-PS1-7

According to the following equation;

C + HNO₃ → CO₂ + NO₂ + H₂O

2.4 grams C is reacted with concentrated HNO₃ acid. How many liters of NO₂ are produced at STP? (C: 12) (Balance the equation first)

• A) 5.6

• B) 11.2

• C) 16.8

• D) 17.92

• E) 22

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-7

For the following balanced chemical equation

2Al(s) + 6HCl(l) → 2AlCl₃(s) + 3H₂(g)

how many moles of H₂ are present?

• 1 mol

• 2 mol

• 3 mol

• 4 mol

• 6 mol

Tags

NGSS.HS-PS1-7

In a stoichiometric calculation to determine the mass of one substance that will react with a given amount, in moles, of a second substance, you need to know

• only the mole ratio of the unknown substance to the given substance.

• only the molar mass of the given substance.

• both the mole ratio of the unknown substance to the given substance and the molar mass of the unknown substance.

• the molar masses of all products and reactants.

Tags

NGSS.HS-PS1-7

Magnesium reacts with hydrochloric acid to produce hydrogen gas and magnesium chloride. How many liters of a 0.750 M HCl solution will react with 12.25 g of Mg?

Mg(s) + 2HCl(aq)→H2(g) + MgCl2(aq)

• 1.34 L

• 2.34 L

• 3.34 L

• 4.34 L