Stoichiometry Lab

You calculated prior to lab that you would obtain 2.44 g of a precipitate. When you weigh your product, you have 1.98 g. What is the percent yield of your product?

• 2.44%

• 1.98%

• 81.1%

• 91.3%

When you calculate the amount of product in a stoichiometry problem, you care calculating the:

• theoretical yield

• actual yield

• percent yield

Tags

NGSS.HS-PS1-7

Given: 4Al _(s) + 3O_{2 (g)} ---> 2Al₂O₃ (s) If you are given 10.0 g of aluminum and 10.0 g of oxygen gas, how many moles of aluminum oxide are produced?

• 0.208 mol

• 0.185 mol

• 0.371 mol

• 0.313 mol

When you weigh the aspirin you made in lab, you get a 53.5% yield. The theoretical yield was 3.50g. What was the actual yield?

• 53.5g

• 3.50g

• 0.534g

• 1.87g

What volume of oxygen gas is produced from 8.50 moles of water?

• 22.4 L

• 95.2 L

• 190. L

• 44.8 L

Tags

NGSS.HS-PS1-7

Given: 3F_{2 (g)} + 2FeCl_{3 (aq)} - - > 2FeF_{3 (s)} + 3Cl_{2 (g)}

195 L of fluorine gas will produce how many moles of iron III chloride?

• 0.115 mol

• 8.71 mol

• 0.172 mol

• 5.80 mol

Mg₃N₂ + 3H₂O ––> 3 MgO + 2NH₃

If 10.3 g of magnesium nitride is used, what volume of ammonia gas would be collected at 20˚C and 0.989 atm?

• 4.9 L NH₃

• 4.96 L NH₃

• 0.261 L NH₃

• 0.26 L NH₃

Hydrochloric acid and magnesium react to produce magnesium chloride and hydrogen gas. As in the molar volume lab, the gas is collected in a tube by water displacement. The space above the water contains

• hydrogen gas only.

• hydrogen gas, water vapor, and magnesium chloride.

• hydrogen gas and water vapor.

• hydrogen gas and magnesium chloride.

Tags

NGSS.MS-PS1-2

NGSS.MS-PS1-5

Hydrogen and oxygen react under a specific set of conditions to produce water according to the follwoing: 2H₂(g) + O₂(g) --> 2H₂O(g). How many moles of hydrogen would be required to produce 5.0 mol of water?

• 5.0 mol H₂

• 4.0 mol H₂

• 7.0 mol H

• 5.0 mol of H

Tags

NGSS.HS-PS1-7

Given the combustion reaction C₃H₈ + 5O₂ ​​→ 3CO₂ + 4H₂O, how many liters of carbon dioxide can be produced from 1.00 liter of O₂ at standard temperature and pressure?

• 0.600 L

• 0.825 L

• 1.21 L

• 1.67 L