Unit 8 Mock Exam

Consider the general balanced equation for a single replacement reaction shown below:

A + 2BC → AC₂ + B₂

If 5.0moles of A are combined with 4.0moles of BC, how many moles of B₂ can form?

• 2.0 moles of B₂

• 5.0 moles of B₂

• 4.0 moles of B₂

• 1.0 moles of B₂

Tags

NGSS.HS-PS1-7

Consider the general balanced equation for a single replacement reaction shown below:

A + 2BC → AC₂ + B₂

The molar mass of B is 10.0grams. If 4.0 moles of A and 3.0 moles of BC are mixed and allowed to react, how many grams of B₂ can form?

• 30.0 grams of B₂

• 40.0 grams of B₂

• 10.0 grams of B₂

• 15.0 grams of B₂

Tags

NGSS.HS-PS1-7

 In the chemical reaction

2H₂O  → 2H₂ + O₂

CHECK ALL THAT APPLY

• twice as much H₂ as O₂ will be produced.

• two moles of water is consumed for every two moles of hydrogen produced.

• twice as much O₂ as H₂ will be produced.

• two moles of water is consumed for every one mole of oxygen produced.

Tags

NGSS.HS-PS1-7

NGSS.HS-PS1-2

If 2.5mol of TiCl₄ and 2.5mol of H₂ is carried out to completion,

TiCl₄ + 2H₂ → Ti + 4HCl

SELECT ALL THAT APPLY

• All of the TiCl₄ is consumed.

• All of the H₂ is consumed.

• 2.5 mol of Ti is produced.

• 5.0 mol of HCl is produced. 

Tags

NGSS.HS-PS1-7

NGSS.HS-PS1-2

How much water could be made from 24 moles of benzene (C₆H₆) by the reaction

2C₆H₆ + 15O₂ → 12CO₂ + 6H₂O

• 72 mol

• 24 mol

• 144 mol

• 8.0 mol

Ammonia (NH₃) is widely used as a fertilizer and in many household cleaners. How much ammonia is produced when 6 mol of hydrogen gas react with an excess of nitrogen gas in a synthesis reaction?

N₂ + 3H₂ → 2NH₃

• 4 mol

• 3 mol

• 9 mol

• Cannot be determined unless the limiting reactant is known

In the chemical reaction

2H₂O  → 2H₂ + O₂

• There is a 2 gram to 1 gram ratio between water and oxygen.

• There is a 2 mol to 1 mol ratio between water and oxygen.

• There are 2 electrons in water for every 1 electron in oxygen.

• The mass of water is twice the mass of oxygen.

Tags

NGSS.HS-PS1-7

Molar mass of Fe₂O₃ = 160. g/mol

Molar mass of CO = 28.0 g/mol

Molar mass of CO₂ = 44.0g/mol

Molar mass of Fe = 55.8g/mol

1 mol = 6.02x10²³ particles

Fe₂O₃(s) + 3CO(g) → 3CO₂(g) + 2Fe(s)

When 400g Fe₂O₃ reacts with excess CO, which of the following could be determined with the information provided?

SELECT ALL THAT APPLY.

• The mass of CO reacted.

• The mass of CO₂ produced.

• The mass of Fe produced.

• The number of atoms Fe produced.

Tags

NGSS.HS-PS1-7

Consider the following reaction:

2NO + O₂ → 2NO₂

How much NO₂ can be produced from 120.g of NO and excess oxygen if the yield is 75.0%?

Molar Mass of NO = 30.0g/mol

Molar Mass of O₂ = 32.0g/mol

Molar Mass of NO₂ = 46.0g/mol

• 138g

• 184g

• 120.g

• 60.0g

Tags

NGSS.HS-PS1-7

 Consider the reaction of CaCN₂ and water to produce CaCO₃ and NH3:

CaCN₂ + 3H₂O → CaCO₃ + 2NH₃

How much NH₃ is produced upon reaction of 160. g of CaCN₂ and 4.0. moles of H₂O?

• 2.00 moles NH₃

• 2.67 moles NH₃

• 4.00 moles NH₃

• 6.00 moles NH₃

Tags

NGSS.HS-PS1-7

NGSS.HS-PS1-2