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Radda [10]
3 years ago
10

If you don't no the answer for sure please don't answee

Chemistry
2 answers:
Nostrana [21]3 years ago
8 0

Answer:

The measurement with three significant figures is 5.60 km.

Explanation:

Significant figures : The figures in a number which expresses the value of the magnitude of a quantity to a specific degree of accuracy is known as significant digits.

Rules for significant figures:

  • Digits from 1 to 9 are always significant and have infinite number of significant figures.
  • All non-zero numbers are always significant. For example: 634, 6.84 and 62.4 all have three significant figures.
  • All zero’s between integers are always significant. For example: 1005, 4.005 and 70.03 all have four significant figures.
  • All zero’s preceding the first integers are never significant. For example: 0.0048 has two significant figures.
  • All zero’s after the decimal point are always significant. For example: 4.300, 95.00 and 150.0 all have four significant figures.
  • All zeroes used solely for spacing the decimal point are not significant. For example : 5000 has one significant figure.

The measurement with three significant figures is 5.60 km.

Where as 0.0005 m has 1 significant figure, 7,077 mg has 4 significant figures and 0.080 mm has 2 significant figures.

FrozenT [24]3 years ago
3 0
The answer is D can I have brainliest
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Ca(OH)2 + H2SO4 ⟶2H2O + CaSO4 What volume of 1.45 M Ca(OH)2 is needed to react with 25.0 moles of H2SO4?
Shkiper50 [21]

Answer:

We need 17.2 L of Ca(OH)2

Explanation:

Step 1: Data given

Concentration of Ca(OH)2 = 1.45 M

Moles of H2SO4 = 25.0 moles

Step 2: The balanced equation

Ca(OH)2 + H2SO4 ⟶2H2O + CaSO4

Step 3: Calculate moles Ca(OH)2

For 1 mol Ca(OH)2 we need 1 mol H2SO4 to produce 2 moles H2O and 1 mol CaSO4

For 25.0 moles H2SO4 we'll need 25.0 moles Ca(OH)2 to produce 50 moles H2O and 25.0 moles CaSO4

Step 4: Calculate volume of Ca(OH)2

Volume Ca(OH)2 = moles Ca(OH)2 / concentration Ca(OH)2

Volume Ca(OH)2 = 25.0 moles / 1.45 M

Volume Ca(OH)2 = 17.2 L

We need 17.2 L of Ca(OH)2

3 0
3 years ago
YOU DO:
mihalych1998 [28]

Answer:

67.1%

Explanation:

Based on the chemical equation, if we determine the moles of sodium carbonate, we can find the moles of NaHCO₃ that reacted and its mass, thus:

<em>Moles Na₂CO₃ - 105.99g/mol-:</em>

6.35g * (1mol / 105.99g) = 0.0599 moles of Na₂CO₃ are produced.

As 1 mole of sodium carbonate is produced when 2 moles of NaHCO₃ reacted, moles of NaHCO₃ that reacted are:

0.0599 moles of Na₂CO₃ * (2 moles NaHCO₃ / 1 mole Na₂CO₃) = 0.1198 moles of NaHCO₃

And the mass of NaHCO₃ in the sample (Molar mass: 84g/mol):

0.1198 moles of NaHCO₃ * (84g / mol) = 10.06g of NaHCO₃ were in the original sample.

And percent of NaHCO₃ in the sample is:

10.06g NaHCO₃ / 15g Sample * 100 =

<h3>67.1%</h3>
7 0
3 years ago
Complete the chart. (Remember to enter a "0" if necessary.)
antoniya [11.8K]
Just remember how many electrons can each sublevel hold.

S=2
P=6
D=10

Since we have 10 for atomic number, we can assume we have 10 electrons

1S2
2S2
2P6
The rest have zero because we already have 10 (2+2+6=10)
3 0
3 years ago
Read 2 more answers
Which of the following measurements is expressed to three significant figures?
Zepler [3.9K]
Which of the following measurements is expressed to three significant figures?
C. 5.60 km
Hope this helps!
5 0
3 years ago
Read 2 more answers
Calculate the number of moles of caco3 (calcium carbonate, or limestone) in a 20.0g sample of this substance
Brrunno [24]
First calculate for the molar mass of the given formula unit, CaCO₃. This can be done by adding up the product when the number of atom is multiplied to its individual molar mass as shown below.

     molar mass of CaCO₃ = (1 mol Ca)(40 g Ca/mol Ca) + (1 mol C)(12 g of C/1 mol of C) + (3 mols of O)(16 g O/1 mol O) = 100 g/mol of CaCO₃

Then, divide the given amount of substance by the calculated molar mass.
            number of moles = (20 g)(1 mol of CaCO₃/100 g)
             number of moles = 0.2 moles of CaCO₃

<em>Answer: 0.2 moles</em>
6 0
3 years ago
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