Question

If 1.5 moles of copper metal reacts 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

Answer 1

@FriedRice is this like the last?

Answer 2

what do you mean is this like the last?

Answer 3

like the last question that you help me with

Answer 4

sure

Answer 5

you have to use molar ratio to find out

Answer 6

is this correct?
balanced equation:
Cu + 2AgNO3 = Cu(NO3)2 + 2Ag

This tells you that 1.5 moles of Cu reacts with 2 moles AgNO3 forming 2 moles silver.
There will be 4.0 - 2.0 moles of excess AgNO3 left over.

Answer 7

if you want to find the excess reagent you will need to balance out the equation

Answer 8

um so is what i said wrong?

Answer 9

what 3 parts?

Answer 10

ok lets start from the biggining

Answer 11

ok

Answer 12

ok tell me what you did

Answer 13

this:
balanced equation:
Cu + 2AgNO3 = Cu(NO3)2 + 2Ag

This tells you that 1.5 moles of Cu reacts with 2 moles AgNO3 forming 2 moles silver.
There will be 4.0 - 2.0 moles of excess AgNO3 left over.

Answer 14

yes

Answer 15

ok then how many moles of Ag can be formed

Answer 16

you might need to you molar ratio to find out how many silvers were formed

Answer 17

hmm. idk how to do that

Answer 18

\(\color{blue}{\text{Originally Posted by}}\) @superhelp101
this:
balanced equation:
Cu + 2AgNO3 = Cu(NO3)2 + 2Ag

This tells you that 1.5 moles of Cu reacts with 2 moles AgNO3 forming 2 moles silver.
There will be 4.0 - 2.0 moles of excess AgNO3 left over.
\(\color{blue}{\text{End of Quote}}\)

Answer 19

Now from the balanced reaction u can see that 1 mole of copper reacts with 2 moles of silver nitrate in order to form one mole of copper nitrate and silver metal

Answer 20

yep

Answer 21

So 1.5 moles of copper metal will need 2\(\times\)1.5= ?? moles of Silver nitrate

Answer 22

3 moles of silver nitrate

Answer 23

\[\frac{ 4.0molesAgNO _{3} }{ 1 } * \frac{ 169.88g AgNO _{3} }{ 1moleAgNO _{3} } *\frac{ 2molesAg }{ 2molesAgNO _{3} }\]

Answer 24

Good, given is 4 moles. So how much reactant will be left. (4-3=?)

Answer 25

1. oooh

Answer 26

Now 1 mole of copper was forming 2 moles of silver element, so 1.5 moles will form ?? moles of silver element.

Answer 27

2\(\times\) 1.5 =?

Answer 28

1mole copper/ 2 silver element = 1.5mole/ x
it is 3

Answer 29

Coppper acts as a \(\bf limiting~reagent\) here. Limiting reagent, also known as the "limiting reactant", is the substance which is totally consumed when the chemical reaction is complete. The amount of product formed is limited by this reagent since the reaction cannot proceed further without it.

Answer 30

So the amount of product formed depends directly on the amount of limiting reagent, in this case copper and not silver nitrate.

Answer 31

\(\color{blue}{\text{Originally Posted by}}\) @superhelp101
1mole copper/ 2 silver element = 1.5mole/ x
it is 3 \(\huge\checkmark\)
\(\color{blue}{\text{End of Quote}}\)

Answer 32

uh uh. Thank y'all!

Answer 33

\(\color{red}{\huge\bigstar}\huge\text{You're Most Welcome! }\color{red}\bigstar\)
\(~~~~~~~~~~~~~~~~~~~~~~~~~~~\color{green}{\huge\ddot\smile}\color{blue}{\huge\ddot\smile}\color{pink}{\huge\ddot\smile}\color{red}{\huge\ddot\smile}\color{yellow}{\huge\ddot\smile}\)

Answer 34

Good job @friedrice !