If 4.8 moles of x and 3.4 moles of y react according to the reaction below, how many moles of the excess reactant will be left over at the end of the reaction? 3x + 2y “yields”/ x3y2 1.7 mol y left over 1.6 mol x left over 0.2 mol y left over 0.1 mol x left over

Answer : The correct option is, 0.2 mole Y left over .

Explanation : Given,

Moles of X = 4.8 mole

Moles of Y = 3.4 mole

The balanced chemical reaction is,

From the balanced reaction, we conclude that

As, 3 moles of X react with 2 moles of Y

So, 4.8 moles of X react with moles of Y

From this we conclude that, the reactant Y is an excess reagent and X is a limiting reagent.

The moles of excess reagent left over at the end of the reaction = Given moles of X - Required moles of X

The moles of excess reagent left over at the end of the reaction = 3.4 - 3.2 = 0.2 mole

Therefore, the moles of excess reagent left over at the end of the reaction is, 0.2 mole Y left over.

The correct answer is : '0.2 mol Y left over'.

Explanation:

Moles of X = 4.8 moles

Moles of Y = 3.4  moles

According to reaction, 3 moles of X react with 2 moles of Y .

Then 4.8 moles of X react with :

moles of Y

Moles of Y reacted = 3.2 moles

Moles of Y left unreacted = 3.4 moles - 3.2 moles = 0.2 moles

As we can see that X is in limiting amount and y is present in an excessive amount.And the left over amount of Y is 0.2 moles.

the correct answer would be d. hope this !

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