Question

If 89.5g of Ag were produced in the following reaction how many grams of Cu reacted?

Cu+2agNO3–>Cu(NO3)2+2Ag
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Answer 1

To solve this problem, we need to use the balanced chemical equation and the molar mass of Cu and Ag to determine the amount of Cu that reacted and the amount of Ag produced.

The balanced chemical equation is:

Cu + 2AgNO3 → Cu(NO3)2 + 2Ag

From the equation, we can see that 1 mole of Cu reacts with 2 moles of Ag to produce 1 mole of Cu(NO3)2 and 2 moles of Ag. This means that the ratio of Cu to Ag in the reaction is 1:2.

To find the amount of Cu that reacted, we can use the ratio of Cu to Ag and the mass of Ag produced:

Molar mass of Cu = 63.55 g/mol

Molar mass of Ag = 107.87 g/mol

Mass of Ag produced = 89.5 g

Number of moles of Ag produced = mass / molar mass = 89.5 g / 107.87 g/mol = 0.829 mol

Since the ratio of Cu to Ag is 1:2, the number of moles of Cu that reacted is half the number of moles of Ag produced:

Number of moles of Cu = 0.829 mol / 2 = 0.4145 mol

To find the mass of Cu that reacted, we can use the number of moles of Cu and the molar mass of Cu:

Mass of Cu reacted = number of moles of Cu × molar mass of Cu = 0.4145 mol × 63.55 g/mol = 26.32 g

Therefore, 26.32 grams of Cu reacted in the reaction.

Step-by-step explanation:

Answer 2

Given:

Mass of Ag produced = 89.5g

We can use the mole ratio of the reaction to calculate the mass of Cu that reacted:

Moles of Ag produced = 89.5g/107.87g/mol = 0.829 mol

Moles of Cu reacted = 0.829 mol/1 mol = 0.829 mol

Mass of Cu reacted = 0.829 mol x 63.55g/mol = 52.5g