untitled

Suppose you want to produce 2.00 L of CO₂ at STP using the reaction below. What mass of sodium bicarbonate (NaHCO₃) should you use?

NaHCO₃ --> Na₂CO₃ + CO₂ + H₂O

Hint: Think about conversion L CO₂ --> ___ --> ___ --> g NaHCO₃

Note: just include the number in your answer

if 10.0 g of ammonium nitrate (NH₄NO₃) is decomposed, what mass of laughing gas (N₂O) will be produced?

___NH₄NO₃  →  ___N₂O  +  ___H₂O

Hint: Think about conversion g NH₄NO₃ --> ___ ---> ___ --> g N₂O

note: answer should only include the number, not the unit

• The mole ratio from the balanced equation

• The Molar Mass of H₂

• The Molar Mass of NH₃

• The mole ratio from the balanced products

Given the following chemical equation 4P + 5O₂ →  2P₂O₅

Which is the correct setup to determine: How many moles of P₂O₅ are formed from 3.4 moles of O₂?

Use Model 1: Mole to Mole

What was given in the example from Model 2? (Hint: did it give you a certain amount of grams or moles

• The mole ratio from the balanced equation

• The Molar Mass of H₂

• The Molar Mass of NH₃

• The molar mass of H₂+H₂

• The molar mass of H₂/H₂