Solution Stoichiometry

In a balanced equation, the ratio between the coeffients of any two substances is called the _______. 

• mole ratio

• stoichiometry

• limiting reactant

• excess reactant

Tags

NGSS.HS-PS1-7

To determine the limiting reactant in a chemical reaction, one must know the

• amount of product formed

• available amount of one of the reactants

• available amount of each of each reactant

• speed of the reaction

Tags

NGSS.HS-PS1-7

A chemical reaction involving substances A and B stops when B is completely used.  B is the

• excess reactant

• primary reactant

• limiting reactant

• primary product

2H₂  +   O₂  →  2H₂O
How many moles of oxygen are consumed if 8 moles H₂ are used?

• 2

• 4

• 6

• 8

Tags

NGSS.HS-PS1-7

For the Balanced Reaction: 3 Mg + 1 Fe₂O₃ → 3 MgO + 2 Fe; What is the ratio of moles of MgO to moles Fe?

• 3mol Mg / 2 mol Fe

• 2 mol Mg/ 3 mol Fe

• 1 mol Fe/ 2 mol Fe

• 3 mol MgO / 2 mol Fe

KClO₃ → 2 KCl + 3 O₂
How many moles of oxygen are produced when 6.7 moles of KClO₃ decompose completely?

• 6.7 mol of O₂

• 1.0 mol of O₂

• 10.1 mol of O₂

• 4.5 mol of O₂

Tags

NGSS.HS-PS1-7

2Na + 2H₂O → 2NaOH+ H₂
How many grams of hydrogen are produced if 120 g of Na are available?

• 5.2 g of H₂

• 2.6 g of H₂

• 690 g of H₂

• 45 g of H₂

Tags

NGSS.HS-PS1-7

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 mass of AgBr is formed when 35.5 mL of 0.184 M AgNO₃ is treated with an excess (extra) of aqueous hydrobromic acid?

• 53.6 g of AgBr

• 1.44 g of AgBr

• 1.23 g of AgBr

• 34.5 g of AgBr

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-7

18.26 mL of a 1.50M HCl reacts with excess (extra) Mg(OH)₂. Calculate the mass of Mg(OH)₂ needed for the reaction.

Mg(OH)₂ + 2 HCl -> 2 H₂O + MgCl₂

• 4.68 g Mg(OH)₂

• 0.798 g Mg(OH)₂

• 0.0274 Mg(OH)₂

• 1.07 g Mg(OH)₂

Tags

NGSS.HS-PS1-7