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jolli1 [7]
3 years ago
12

If you have 9900 g of donuts, how many donuts do you have if each donut has a mass of 150 g?

Chemistry
1 answer:
AlexFokin [52]3 years ago
8 0

You would have 66 donuts.


If each you have 9900g of donuts and each donut has a mass of 150g, we can divide 9900 by 150 to figure out how many donuts we have. To do this, we first have to figure out how many times 150 goes into 990. It goes into 6 times and has a remainder of 90. Now we have to figure out how many times 150 goes into 900. It goes in 6 times, meaning that our answer is 66 donuts.

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How many grams of zinc would be required to produce 9.65g of zinc hydroxide
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The question is incomplete, here is the complete question:

How many grams of zinc would be required to produce 9.65g of zinc hydroxide

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<u>Answer:</u> The mass of zinc required is 6.35 grams

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}     .....(1)

Given mass of zinc hydroxide = 9.65 g

Molar mass of zinc hydroxide = 99.4 g/mol

Putting values in equation 1, we get:

\text{Moles of zinc hydroxide}=\frac{9.65g}{99.4g/mol}=0.0971mol

The given chemical equation follows:

Zn+2MnO_2+H_2O\rightarrow Zn(OH)_2+Mn_2O_3

By Stoichiometry of the reaction:

1 mole of zinc hydroxide is produced from 1 mole of zinc

So, 0.0971 moles of zinc hydroxide will be produced from = \frac{1}{1}\times 0.0971=0.0971mol of zinc

Now, calculating the mass of zinc from equation 1, we get:

Molar mass of zinc = 65.4 g/mol

Moles of zinc = 0.0971 moles

Putting values in equation 1, we get:

0.0971mol=\frac{\text{Mass of zinc}}{65.4g/mol}\\\\\text{Mass of zinc}=(0.0971mol\times 65.4g/mol)=6.35g

Hence, the mass of zinc required is 6.35 grams

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3 years ago
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