Emperical Formula of Copper Oxide

Experiment 2: What was the identity of the precipitate that formed upon the addition of NaOH?

copper hydroxide

Experiment 1: What was the color of the copper before heating?

red-orange

Experiment 1: What was the mass of the copper oxide after heating? Choose the closest answer.

12.518g

Experiment 1: What is the molar ratio of copper to oxygen in the copper oxide formed?

1:1

Experiment 1: The copper changed to copper oxide upon heating. How many grams of oxygen were used in the reaction? Choose the closest answer.

2.518g

How many grams of copper(II) sulfate pentahydrate were added to the beaker? Note: The amount of materials dispensed can vary. Choose the answer that is closest to yours.

25.000g

Experiment 1: What was the mass of the empty crucible? Note: The size of containers in the lab can vary. Pick the answer that is closest to yours.

35.000g

Experiment 1: What was the mass of the crucible after the addition of copper? Choose the closest value.

45.000g

What happened when NaOH was added to the copper(II) sulfate pentahydrate solution?

A blue precipitate formed

Experiment 1: What was the color of the copper oxide after heating?

black

Experiment 2: What color was the copper (II) sulfate pentahydrate before heating?

blue

How many moles of copper(II) sulfate pentahydrate were used in the reaction? The molar mass of copper(II) sulfate pentahydrate is 249.68 g/mol. For best accuracy, use the mass measured with the balance during the experiment. Choose the closest answer.

0.1001 moles

Based on the mass of oxygen in copper oxide, how many moles of oxygen are present? The molar mass of oxygen is 16.00 g/mol.

0.1574 mol

Experiment 1: The molar mass of copper is 63.55 g/mol. How many moles of copper were reacted?

0.1574 mol

Suppose you were to heat the copper in argon gas instead of atmospheric gases. Given that argon is relatively inert, which of the following would you expect if you were to heat pure copper in the presence of argon gas?

Copper oxide would not form and the mass would not change

What is the empirical formula of copper oxide based on your results in Experiment 1?

CuO

Lithium is the only metal that reacts with nitrogen gas at room temperature to form lithium nitride. To avoid oxide formation, the reaction is performed under pure nitrogen gas. Given the experimental data in the table below, what is the empirical formula of lithium nitride? The molar mass of lithium is 6.94 g/mol and that of nitrogen is 14.01 g/mol

Li3N