mole-to-mole conversions\n\nconsider the following unbalanced chemical equation: $cu + agno_3 \\rightarrow…

mole-to-mole conversions\n\nconsider the following unbalanced chemical equation: $cu + agno_3 \\rightarrow cu(no_3)_2 + ag$\n\nhow many moles of silver nitrate are needed to produce 3.415 moles of copper(ii) nitrate?\n\\boxed{} moles of $cu$\n\n*please report your answer to the appropriate number of significant figures.

mole-to-mole conversions\n\nconsider the following unbalanced chemical equation: $cu + agno_3 \\rightarrow cu(no_3)_2 + ag$\n\nhow many moles of silver nitrate are needed to produce 3.415 moles of copper(ii) nitrate?\n\\boxed{} moles of $cu$\n\n*please report your answer to the appropriate number of significant figures.

Answer

Explanation:

Step1: Balance the chemical equation

$\text{Cu} + 2\text{AgNO}_3 \rightarrow \text{Cu(NO}_3\text{)}_2 + 2\text{Ag}$

Step2: Identify mole ratio

From the balanced equation, the mole ratio of $\text{AgNO}_3$ to $\text{Cu(NO}_3\text{)}_2$ is $\frac{2\ \text{mol AgNO}_3}{1\ \text{mol Cu(NO}_3\text{)}_2}$

Step3: Calculate moles of $\text{AgNO}_3$

$3.415\ \text{mol Cu(NO}_3\text{)}_2 \times \frac{2\ \text{mol AgNO}_3}{1\ \text{mol Cu(NO}_3\text{)}_2}$

Answer:

6.830 moles of $\text{AgNO}_3$