If 1.5 moles of copper metal react with 4.0 moles of silver nitrate, how many moles of silver metal can be formed, and how many moles of the excess reactant will be left over when the reaction is complete? unbalanced equation: cu + agno3 → cu(no3)2 + ag .

1 mole of excess reactant (AgNO will be left.

Step-by-step explanation:

First of all, we need to balance the given equation to get:

2 → 2

We know that,

1 mole of Cu reacts with 2 moles of AgNO

So supposing the number of moles of AgNO to be x for 1.5 moles of Cu, we can find x:

Therefore 3 moles of AgNO are needed to complete the reaction while we have excess of it (4 moles). So 1 mole of excess reactant AgNOwill be left.

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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