# Avogadro’s Number 6 022 x 10^23

Copper + Silver(I) Nitrate → Copper(II) Nitrate + Silver

1.

Question

# Avogadro’s Number 6.022 x 10^23 Copper + Silver(I) Nitrate → Copper(II) Nitrate + Silver 1.

Using chemical formulas, write out the balanced chemical equation for the reaction above.

2. Using a periodic table, find all the molar masses of the compounds

3. If the density of copper is 8.96 g/cm^3, what is the mass of 14.68 mL copper? Show your answer in kilograms.

4. How many molecules of Silver(I) Nitrate does it take to produce 21.8g Silver?

5. When you react 28.7g Copper with 36.4g Silver(I) Nitrate, how many grams Copper(II) Nitrate should be produced? (Hint: find the limiting reagent

6. When you react the masses from Question 5 in a lab, you produce 16.5g Copper(II) Nitrate. What is the percent yield for the reaction

7. How many grams oxygen are in 6.7g Copper(II) Nitrate? What is the percent by mass? 21)

15) The ratio of the mass of oxygen that combines with 1.0 g of hydrogen in water to the mass of oxygen that combines with 1.0 g of hydrogen in hydrogen peroxide is 1:2. Taken by itself, this fact demonstrates what natural law? a. Definite proportions b. Conservation of Mass c. Muiple proportions d. The Atomic Theory

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