5th Six Weeks Re-Test

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

• SO

• SO₂

• SO₃

• SO₄

What is the molecular formula for a compound with the empirical formula: K₂SO₄ and a molecular mass of 696g.

• K₂SO₄

• K₈SO₁₆

• K₈S₄O₈

• K₈S₄O₁₆

Balance this equation.
_SnO₂ +_H₂-->_Sn +_H₂O

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

Balance this equation
_Al +_HCl --> _H₂ +_AlCl₃

• 2, 6, 3, 2
• it is already balanced
• 4, 12, 3, 4
• 2, 1, 4, 5

Identify the type of chemical reaction (a)  

• Synthesis
• Decomposition
• Single replacement
• Double replacement
• Combustion

Identify the type of chemical reaction

• Synthesis

• Decomposition

• Single replacement

• Double replacement

• Combustion

1 CH₄ + 2 O₂ → 1 CO₂ + 2 H₂O

How many moles of carbon dioxide (CO₂) are produced from the combustion of 110.0 g of CH₄ (molar mass = 16 g)?

• 13.7 mol

• 2.75 mol

• 6.85 mol

• 6.11 mol

Tags

112.43.c.9.C

2 Al₂O₃ → 4 Al + 3 O₂

Calculate the moles of aluminum (Al) from 5.00 mol of aluminum oxide (Al₂O₃).

• 7.5 mol

• 10 mol

• 2.5 mol

• 4 mol

Tags

112.43.c.9.C

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

• 2
• 4
• 6
• 8

CH₄ + 2 O₂ → CO₂ + 2 H₂O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH₄?

• 13.7 mol
• 2.75 mol
• 6.11 mol
• 6.85 mol