Stoichiometry 2

2NaN₃ → 2Na + 3N₂

How many grams of NaN₃ are needed to produce 10.0 L of N₂ at 1.50 atm and 25.0°C?

• 20.5 g

• 32.8 g

• 15.0 g

• 26.5 g

Tags

NGSS.HS-PS1-7

NGSS.HS-PS1-5

2CO + O₂ → 2CO₂

How many moles of carbon monoxide are needed to react with 12.30 L of oxygen gas at STP?

• 3.149 mol CO

• 31.80 mol CO

• 1.098 mol CO

• 20.10 mol CO

What is the volume occupied by one mole of an ideal gas at standard temperature and pressure (STP)?

• 6.022x10^23

• 1

• Molar Mass

• 22.4 liters

What is the term for the mass of one mole of a substance?

• Avogadro's Number

• Atomic Mass

• Molar Mass

• Mole Fraction

Given the equation:

2NaClO₃ (s) → 2NaCl (s) + 3O₂ (g)

When 2.00 moles of NaClO₃ react, how many grams of O₂ is produced?

• 56 g of O₂

• 96 g of O₂

• 64 g O₂

• 32 g O₂

Tags

NGSS.HS-PS1-7

In a chemical reaction, which numbers indicate the proportions of reactants and products?

• Subscripts

• Superscripts

• Coefficients

Tags

NGSS.HS-PS1-7

Using the following equation:
2KClO₃(s) → 2KCl(s) + 3O₂(g)
How many moles of oxygen gas can be produced from 8 moles of KClO₃? 

• 12 moles O₂

• 8 moles O₂

• 6 moles O₂

• 4 moles O₂

Tags

NGSS.HS-PS1-7

2 KClO₃ (s) → 2KCl (s) +3 O₂ (g)

How many grams of O₂ will be produced from 10.00 moles of KClO₃?

• 240 g of O₂

• 480 g of O₂

• 320 g O₂

• 160 g O₂

How do you calculate the molar mass of a compound?

• By adding up the molar masses of its component elements

• By dividing the molar mass of the compound by the number of moles

• By multiplying the molar mass of the compound by Avogadro's number

• By subtracting the molar mass of the compound from the molar mass of carbon-12

A limiting reactant is a reactant that.....

• runs out during a chemical reaction

• causes a reaction to stop

• determines the amount of products that can be made

• all of these