Question

The exothermic reaction between solid aluminium powder and solid manganese (IV) oxide, produces solid manganese and
another product. How many moles of aluminium powder are needed to produce 203.7 grams of manganese?

Answer 1

The number of moles of aluminum powder needed to produce 203.7 grams of manganese is 5 moles.

How to calculate the number of moles of Aluminium powder?

Heat, Mn, and Al2O3 are produced when aluminum powder and manganese dioxide are heated.

$3MnO_{2} + 4Al - > 3Mn + 2Al_{2} O_{3} + Heat$

The balanced chemical equation in this situation indicates that there are 3 moles of manganese and 4 moles of aluminum involved in the reaction, which results in a 3:4 mole ratio.

You may make use of this mole ratio by calculating how many moles of aluminum are required to react with the 203.7g of Manganese. So,

Firstly, the mass of Aluminium has to be taken out

Let the mass be considered x.

So, the number of moles of Aluminium = x/27

Number of moles of Manganese = 203.7/54

Hence, the mass x will be,

$x = 4 *203.7 * 27 / 3 * 54$

$x = 135.8g$

Hence,  the number of moles of Aluminium is = 135.8/27 = 5 moles.

To learn more about the Calculation of a number of moles refer to:

https://brainly.com/question/15321053

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