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Free_Kalibri [48]
3 years ago
6

Determine the percent error if a student determines that the mass of a block is 45.6 grams and the actual mass is 46.7g.

Chemistry
2 answers:
Charra [1.4K]3 years ago
3 0

Answer:

<h2>2.36 %</h2>

Explanation:

The percentage error of a certain measurement can be found by using the formula

P(\%) =  \frac{error}{actual \:  \: number}  \times 100\% \\

error = 46.7 - 45.6 = 1.1

actual mass = 46.7

From the question we have

p(\%) =  \frac{1.1}{46.7}  \times 100 \\  = 2.3555...

We have the final answer as

<h3>2.36 %</h3>

Hope this helps you

Alina [70]3 years ago
3 0

Answer:

2.36%

Explanation:

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6.0 mol Al reacts with 4.0 mol O2 to form Al2O3.
Tema [17]

Answer:

3.0 moles Al₂O₃

Explanation:

We do not know which of the reactants is the limiting reactant. Therefore, you need to convert both of the given mole values into the product. This can be done using the mole-to-mole ratio made up of the balanced equation coefficients.

4 Al + 3 O₂ -----> 2 Al₂O₃

6.0 moles Al            2 moles Al₂O₃
----------------------  x  -------------------------  =  3.0 moles Al₂O₃
                                    4 moles Al

4.0 moles O₂           2 moles Al₂O₃
----------------------  x  -------------------------  =  2.7 moles Al₂O₃
                                    3 moles O₂

As you can see, O₂ produces the smaller amount of product. This means O₂ is the limiting reactant. Remember, the limiting reactant is the reactant which runs out before the other reactant(s) are completely reacted. As such, the actual amount of Al₂O₃ produced is 2.7 moles.

However, since this problem is directly addressing how much Al₂O₃ is produced from Al, the answer you most likely are looking for is 3.0 moles Al₂O₃.

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