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bogdanovich [222]
3 years ago
14

Which of the following examples illustrates a number that is correctly rounded to three significant figures?

Chemistry
1 answer:
Naily [24]3 years ago
8 0

Answer:

c. 20.0332 g to 20,0 g

Explanation:

A significant figure is each of the digits of a number that are used to express it to the required degree of accuracy, starting from the first non-zero digit, with the exception of the trailing zeros.

<em>Which of the following examples illustrates a number that is correctly rounded to three significant figures? </em>

a. 109 526 g to 109 500 g. NO. The rounded number has 4 significant figures: 109 500.

b. 0.03954 g to 0.040 g. NO. The rounded number has 2 significant figures:  0.040.

c. 20.0332 g to 20.0 g. YES. The rounded number has 3 significant figures:  20.0.

d. 04.05438 g to 4.054 g. NO. The rounded number has 4 significant figures: 4.054.

e. 103.692 g to 103.7g. NO. The rounded number has 4 significant figures: 103.7.

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What volume would 3.00 moles of neon gas have at 295 K and 645 mmHg?
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The reaction of 4.8g of sulfur and 5.4g aluminum yields 4.5g Al2S3. 3S+2AL--&gt;Al2S3 Determine the percent yield of Al2S3.
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Answer:

59.9% is the percent yield for the 4.5 g of produced Al₂S₃

Explanation:

Let's determine the reaction:

3S  +  2Al  →  Al₂S₃

First of all, let's determine the limiting reactant. We need to convert the mass to moles:

4.8 g /32.06g/mol = 0.150 moles of S

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3 moles of S react to 2 moles of Al

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2 moles of Al react to 3 moles of S

Then 0.2 moles of Al may react to (0.2 . 3) /2 = 0.3 moles of S. (We only have 0.150 moles)

Let's go to the product, 3 moles of S can produce 1 mol of Al₂S₃

Then 0.150 moles of S, may produce (0.150 . 1) /3 = 0.05 moles.

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0.05 mol . 150.15g /mol =  7.50g

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% = (4.5g / 7.5g) . 100 = 59.9%

8 0
3 years ago
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