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Kryger [21]
3 years ago
9

The volume of solution in a test tube is measured to be 0.0067 liter. Which digits in the measurement are significant figures?

Chemistry
2 answers:
puteri [66]3 years ago
8 0

<u>Given data:</u>

Volume of solution measured = 0.0067 L

<u>To determine:</u>

The number of significant figures

<u>Explanation:</u>

Significant figures are the number of digits that accurately describe a measured value.

As per the rules:

All non-zero digits are significant

Leading zero's i.e. the zero's after a decimal which comes before a non-zero digit are not significant

Hence in the given value 0.0067, there are 2 significant figures (6 &7)


frozen [14]3 years ago
6 0

Answer:

Digits in the measurement are significant figures are '6' and '7'.

Explanation:

Significant figures : The figures in a number which express the value -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: 604, 6.49 and 65.4 all have three significant figures.

All zero’s between integers are always significant. For example: 5005, 4.805 and 50.06 all have four significant figures.

All zero’s preceding the first integers are never significant. For example: 0.0058 has two significant figures.

All zero’s after the decimal point are always significant. For example: 4.500, 47.00 and 550.0 all have four significant figures.

Significant figures in measurement 0.0067 liter = 2

Digits in the measurement are significant figures are '6' and '7'.

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A balloon filled with helium occupies 20.0 l at 1.50 atm and 25.0◦c. How many moles of helium will there be in the balloon at st
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Answer:

  • There will be 1.23 moles of helium in the balloon at STP

Explanation:

1) <u>Initial conditions of the helium gas</u>:

  • V = 20.0 liter
  • p = 1.50 atm
  • T = 25.0 °C = 25.0 + 273.15 K = 298.15 K

2) <u>Ideal gas equation</u>:

  • pV = n RT
  • p, V, and T are given above
  • R is the Universal constant = 0.0821 atm-liter / ( K - mol)
  • n is the unknown number of moles

3) <u>Solve for n</u>:

  • n = pV / (RT) =
  • n = 1.50 atm × 20.0 liter / (0.0821 atm-liter /k -mol ×298.15K)
  • n = 1.23 mol

4) <u>At STP:</u>

  • STP stands for standard pressure and temperature.
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A 4.00L flask containing Ne at 25 C and 6.00 atm is joined by a valve to an 8.00 L flask Ar at 25 C and 2.00 atm.
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Answer:

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Explanation:

Hello!

In this case, since know the volume, temperature and pressure of the initial containers, we can compute the moles of each gas prior to the opening of the valve as shown below:

n_{Ne}=\frac{6atm*4L}{0.08206\frac{atm*L}{mol*K}*298.15K} =0.981molNe\\\\n_{Ar}=\frac{2atm*8L}{0.08206\frac{atm*L}{mol*K}*298.15K} =0.654molAr

Next, we add them up to obtain the total moles:

n_T=0.981mol+0.654mol=1.635mol

Now, the total volume:

V_T=4.00L+8.00L=12.00L

Finally, the total pressure is computed by using the ideal gas equation:

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Best regards!

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