How many moles of silver nitrate are needed to produce 6.75 moles of copper nitrate (CU(NO3)2) upon reaction with excess copper by useing this equation:

2AgNO3(Aq) + Cu (s)-->2Ag(s)+Cu(NO3)2 (AQ)

To determine the number of moles of silver nitrate (AgNO3) needed to produce 6.75 moles of copper nitrate (Cu(NO3)2), we need to use the balanced chemical equation:

2AgNO3(Aq) + Cu (s) --> 2Ag(s) + Cu(NO3)2 (AQ)

From the equation, we can see that the ratio between silver nitrate and copper nitrate is 2:1. This means that for every 2 moles of AgNO3, we will produce 1 mole of Cu(NO3)2.

To find the number of moles of silver nitrate needed, we can use the following equation:

moles of AgNO3 = moles of Cu(NO3)2 / (2/1)

Substituting the given value:

moles of AgNO3 = 6.75 / (2/1)
= 6.75 * (1/2)
= 3.375 moles

Therefore, 3.375 moles of silver nitrate (AgNO3) are needed to produce 6.75 moles of copper nitrate (Cu(NO3)2) in the given reaction.

To determine how many moles of silver nitrate (AgNO3) are needed to produce 6.75 moles of copper nitrate (Cu(NO3)2), we need to first examine the balanced chemical equation:

2AgNO3(aq) + Cu(s) -> 2Ag(s) + Cu(NO3)2(aq)

From the equation, we can see that the mole ratio between AgNO3 and Cu(NO3)2 is 2:1. This means that for every 2 moles of AgNO3, we will produce 1 mole of Cu(NO3)2.

To find the moles of AgNO3 needed, we can set up a proportion using the mole ratio:

2 moles AgNO3 / 1 mole Cu(NO3)2 = x moles AgNO3 / 6.75 moles Cu(NO3)2

Cross-multiplying the proportion gives:

2 moles AgNO3 * 6.75 moles Cu(NO3)2 = x moles AgNO3 * 1 mole Cu(NO3)2

Simplifying the equation, we have:

13.5 moles AgNO3 = x moles AgNO3

Therefore, you would need 13.5 moles of silver nitrate to produce 6.75 moles of copper nitrate during the reaction.

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How many moles of silver nitrate are needed to produce 6.75 moles of copper nitrate (CU(NO3)2) upon reaction with excess copper by useing this equation:

2AgNO3(Aq) + Cu (s)-->2Ag(s)+Cu(NO3)2 (AQ)