Copper reacts with silver nitrate to produce silver and copper(II) nitrate according to the equation below: Cu + 2AgNO3 →Cu(NO3)2 + 2Ag Calculate the number of moles of copper(II) nitrate produced when 5 moles of copper react. Type your answer as a number with 1 significant figure. Make sure to include the correct units in your answer. Units are a type of measurement i. e. gram (g) or mole (mol). Do not include the chemical formula in your answer.

of would be produced (assuming that reaction does not run out of until all the was converted.)

Explanation:

Make sure that the equation for this reaction is indeed balanced:

.

The coefficient of and are not shown. That implies that the coefficient of both species would be . In other words, the actual equation for this reaction should be:

.

Coefficient of in this equation: .

Coefficient of in this equation: .

Thus, the ratio between the coefficient of and that of would be .

Assume that is the limiting reactant of this reaction (that is: this reaction runs out of before running out of any other reactant.) This coefficient ratio would be equal to the ratio between:

Hence, under the assumption that is the limiting reactant:

.

The question states that of was available. That is: . Assume that is indeed the limiting reactant.

.

Hence, under this assumption, of would be produced.

if the concentration of products is decreased, the equilibrium will shift toward the products). add an inert gas (one that is not involved in the reaction) to the constant-volume reaction mixture: this will increase the total pressure of the system, but will have no effect on the equilibrium condition.

explanation: