Mole calculations Practice

Balance the following reaction:
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)

• 1,2,1,2
• 2,1,1,2
• 1,2,1,1
• 1,2,2,2

Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?

• 5.00 g
• 7.29
• 182 g
• 218 g

Tags

NGSS.HS-PS1-7

Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
What mass of H₂ gas is formed when 4.0 moles of HCl is fully reacted with excess Mg?

• 0.99 g
• 4.0 g
• 2.0 g
• 6.0 g

Tags

NGSS.HS-PS1-7

Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   + H₂(g)
How many moles of HCl are consumed in the production of 7.5 moles of MgCl₂?

• 3.8 moles
• 15 moles
• 7.5 moles
• 23 moles

Tags

NGSS.HS-PS1-7

Balance the following reaction :
 CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)

• 1,2,2,2
• 1,2,1,1
• 2,1,1,1
• 2,1,2,1

Tags

NGSS.HS-PS1-7

 Using the balanced equation in question 5, CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
how many grams of H₂O are needed if 3.20 moles of CaC₂ are used up?

• 115 g
• 28.8 g
• 0.0889 g
• 6.40 g

Tags

NGSS.HS-PS1-7

Using the balanced equation in question 5,
 CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
how many grams of Ca(OH)₂ would be formed by using up 3.20 moles of CaC₂?

• 119 g
• 21.2 g
• 114 g
• 237 g

Tags

NGSS.HS-PS1-7

Using the balanced equation in question 5,
 CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
how many moles of Ca(OH)₂ would be produced if 3.5 moles of H₂O are consumed?

• 1.75 moles
• 7.0 moles
• 3.5 moles
• 11 moles

Tags

NGSS.HS-PS1-7

Balance the following reaction:  
C₂H₂(g) + O₂(g) --> CO₂(g) + H₂O(g)

• 4,10,2,1
• 2,5,4,2
• 1,2,2,1
• 4,10,2,2

Using the balanced equation in question 9,
C₂H₂(g) + O₂(g) --> CO₂(g) + H₂O(g)C₂H₂(g) + O₂(g) --> CO₂(g) + H₂O(g)
How many moles of water (H₂O) are produced when 25.0 grams of C₂H₂ are consumed?

• 0.960 moles
• 0.480 moles
• 1.92 moles
• 3.84 moles