Final Exam Review Part 1

Calculate the number of moles in 1.75 x10²⁴ formula units of NaCl.

• 1.05x10⁴⁸ mol NaCl

• 2.91 mol NaCl

• 5.81 mol NaCl

• 2.10x10⁴⁸ mol NaCl

Tags

NGSS.HS-PS1-7

Calculate the number of molecules in 2.35 moles of CO.

• 1.41x10²⁴ molecules CO

• 3.90x10^-24 molecules CO

• 7.80x10^-24 molecules CO

• 2.82x10²⁴ molecules CO

The molar mass of water is 18.02 g/mol. How many moles is in 70.0 g of water?

• 3.88 mol

• 1261.4 mol

• 11.65 mol

• 1.29 mol

What is the definition of molar mass?

• number of grams per one mole of a substance
• whole number ratio that is a multiple of a chemical formula
• simplest, whole number ratio of a chemical formula
• 6.02 x 10^23 particles per one mole of a substance

What is the molar mass of AuCl₃?

• 96 g
• 130 g
• 232.5 g
• 303.3 g

Which would have more atoms?

• 1 mole of Li
• 1 mole of Au
• 1 mole of Si
• None, all are equal

How many moles are present in 32.3 grams of carbon dioxide (CO₂)?

• 44.01 moles
• 1421.52 moles
• 32.3 moles
• 0.73 moles

Tags

NGSS.HS-PS1-7

What is the molar mass of C₆H₁₂O₆?

• 180.18 g/mol

• 180.12 g/mol

• 180.24 g/mol

• 180.06 g/mol

Using the following equation:
Fe₂O₃(s) + 3H₂(g) → 2Fe(s) + 3H₂O(l)
How many moles of iron can be made from  6 moles H₂? 

• 4 moles Fe
• 6 moles Fe
• 9 moles Fe
• 2 moles Fe

Tags

NGSS.HS-PS1-7

2 NaClO₃ (s) --> 2NaCl (s) +3 O₂ (g)  
12.00 moles of NaClO₃ will produce how many grams of O₂?

• 256 g of O₂
• 576 g of O₂
• 288 g O₂