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The question is incomplete, here is the complete question:
When silver nitrate reacts with copper, copper(II) nitrate and silver are produced. The balanced equation for this reaction is:
Suppose 6 moles of silver nitrate react. The reaction consumes___ moles of copper. The reaction produces __ moles of copper(II) nitrate and __ moles of silver.
<u>Answer:</u> The amount of copper metal reacted is 3 moles, amount of copper (II) nitrate produced is 3 moles and amount of silver metal produced is 6 moles.
<u>Explanation:</u>
We are given:
Moles of silver nitrate = 6 moles
For the given chemical reaction:
- <u>For copper metal:</u>
By Stoichiometry of the reaction:
2 moles of silver nitrate reacts with 1 mole of copper metal
So, 6 moles of silver nitrate will react with = of copper metal
Moles of copper reacted = 3 moles
- <u>For copper(II) nitrate:</u>
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 1 mole of copper(II) nitrate
So, 6 moles of silver nitrate will produce = of copper(II) nitrate
Moles of copper(II) nitrate produced = 3 moles
- <u>For silver metal:</u>
By Stoichiometry of the reaction:
2 moles of silver nitrate produces 2 moles of silver metal
So, 6 moles of silver nitrate will produce = of silver metal
Moles of silver metal produced = 3 moles
Hence, the amount of copper metal reacted is 3 moles, amount of copper (II) nitrate produced is 3 moles and amount of silver metal produced is 6 moles.
Answer: Molar mass of is 17.03 g
Explanation:
Molar mass is defined as the mass in grams of 1 mole of a substance.
S.I Unit of Molar mass is gram per mole and it is represented as g/mol.
It is found by adding the atomic masses of all the elements present.
Atomic Mass of Nitrogen (N) = 14.007 g
Atomic Mass of Hydrogen (H) = 1.008 g
Molar mass of = 1(14.007)+3(1.008) g = 17.03 g