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Misha Larkins [42]
3 years ago
9

Choose the number of significant figures 60.0

Chemistry
2 answers:
GenaCL600 [577]3 years ago
8 0

Answer:

3 significant figures

Explanation:

The rules for deciding which digits in a measurement are significant are as follows:

1) All nonzero digits are significant.

2) Sandwiched (or embedded) zeros, those between significant digits, are significant.

3) Leading zeros, which are zeros at the beginning of a decimal number less than 1, are not significant.

4) Trailing zeros, which are zeros at the end of a number, are significant only if the number has a decimal point.

By rule 4 since 60.0 has a decimal point all 3 figures are significant

oksian1 [2.3K]3 years ago
4 0

 

In this case there are 3 significant figures.

Any zeroes after another number, (i.e. 9300.000), you consider these numbers.  

If there is something like 0.0060, this would be two significant digits.  

Zeroes before a number are not significant, anything after are.  

Hope this helps any confusion!


Please mark me brainliest!

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A chemist determined by measurements that 0.050 moles of aluminum participated in a chemical reaction. Calculate the mass of alu
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Answer:

13.5 g

Explanation:

This question is solved easily if we remember that the number of moles is obtained by dividing the mass into the atomic weight or molar mass depending if we are referring to elements or molecules.

Therefore, the mass of aluminum in the reaction will the 0.050 mol Al times the atomic weight of aluminum.

number of moles = n = mass of Al / Atomic Weight Al

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From the ionization of H₂SO₄, we have

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That is; 0.250·H₂SO₄ → 0.5·H⁺ + 0.250·SO₄²⁻.

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