How many moles of Cu are needed to react with 3.50 moles of AgNO3?
To answer this question, you need to know the balanced chemical equation for the reaction between copper (Cu) and silver nitrate (AgNO3).
The balanced equation is:
Cu + 2AgNO3 → Cu(NO3)2 + 2Ag
From the equation, you can see that 1 mole of Cu reacts with 2 moles of AgNO3.
To calculate the number of moles of Cu needed to react with 3.50 moles of AgNO3, you can use the mole ratio from the balanced equation.
Mole ratio: 1 mole of Cu reacts with 2 moles of AgNO3
So, for every 2 moles of AgNO3, you need 1 mole of Cu.
To find the number of moles of Cu needed when you have 3.50 moles of AgNO3, you can set up a proportion:
(1 mole of Cu / 2 moles of AgNO3) = (x moles of Cu / 3.50 moles of AgNO3)
Solving for x, you get:
x = (1 mole of Cu / 2 moles of AgNO3) * (3.50 moles of AgNO3)
Calculating this, you will find:
x = 1.75 moles of Cu
Therefore, you would need 1.75 moles of Cu to react with 3.50 moles of AgNO3.
To determine the number of moles of Cu needed to react with AgNO3, we must first balance the chemical equation for the reaction between Cu and AgNO3. The balanced equation is:
Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag
From the balanced equation, we can see that 1 mole of Cu reacts with 2 moles of AgNO3.
Given that there are 3.50 moles of AgNO3, we can set up a proportion to determine the number of moles of Cu:
1 mole Cu / 2 moles AgNO3 = x moles Cu / 3.50 moles AgNO3
Cross multiplying the proportion, we have:
2 moles AgNO3 * x moles Cu = 1 mole Cu * 3.50 moles AgNO3
Simplifying the equation, we get:
2x = 3.50
Dividing both sides of the equation by 2, we find:
x = 1.75
Therefore, we need 1.75 moles of Cu to react with 3.50 moles of AgNO3.
Cu + 2AgNO3-->Cu(NO3)2+ 2Ag
3.50/2 <--3.50