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liq [111]
3 years ago
11

the student measured the volume of water as 80.0 mL. she discovered that the actual volume was 80.1 mL. is her results ac urate

why or why not

Chemistry
2 answers:
Oksana_A [137]3 years ago
8 0
Yes, the more decimal places in a number mean that it is more accurate :3
adoni [48]3 years ago
8 0

<u>Answer:</u> The result of the student measured is not accurate.

<u>Explanation:</u>

Accuracy is defined as the closeness of a measured value to a standard or known value.

For Example: If the mass of a substance is 50 kg and one person weighed 48 kg and another person weighed 55 kg. Then, the weight measured by first person is more accurate.

Precision is defined as the closeness of two or more measurements to each other.

For Example: If you weigh a given substance five times and you get 1.8 kg each time. Then the measurement is said to be precise.

Level of precision is determined by the maximum number of decimal places.

We are given:

Actual volume = 80.1 mL

Measured value = 80.0 mL

As, the measure value is 0.1 mL less than the true value. The level of precision is very high in this case. So, the measured value is not accurate.

Hence, the result of the student measured is not accurate.

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A hypothetical element has an atomic weight of 48.68 amu. It consists of three isotopes having masses of 47.00 amu, 48.00 amu, a
Morgarella [4.7K]

Answer : The percent abundance of the heaviest isotope is, 78 %

Explanation :

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i

As we are given that,

Average atomic mass = 48.68 amu

Mass of heaviest-weight isotope = 49.00 amu

Let the percentage abundance of heaviest-weight isotope = x %

Fractional abundance of heaviest-weight isotope = \frac{x}{100}

Mass of lightest-weight isotope = 47.00 amu

Percentage abundance of lightest-weight isotope = 10 %

Fractional abundance of lightest-weight isotope = \frac{10}{100}

Mass of middle-weight isotope = 48.00 amu

Percentage abundance of middle-weight isotope = [100 - (x + 10)] %  = (90 - x) %

Fractional abundance of middle-weight isotope = \frac{(90-x)}{100}

Now put all the given values in above formula, we get:

48.68=[(47.0\times \frac{10}{100})+(48.0\times \frac{(90-x)}{100})+(49.0\times \frac{x}{100})]

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Therefore, the percent abundance of the heaviest isotope is, 78 %

5 0
3 years ago
Read 2 more answers
What is the mole fraction of O2O2 in a mixture of 15.1 gg of O2O2, 8.19 gg of N2N2, and 2.46 gg of H2H2
SVETLANKA909090 [29]

Answer:

Mole fraction O₂=  0.43

Explanation:

Mole fraction is the moles of gas/ total moles.

Let's determine the moles of each:

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Moles N₂  →  8.19 g / 14 g/mol = 0.013

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Total moles = 2.183

Mole fraction O₂= 0.94 / 2.183 → 0.43

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ikadub [295]

Answer:

See explanation

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As the distance of separation between atoms decreases, the potential energy of the system decreases accordingly.

An optimum distance is reached when the two atoms attain the lowest potential energy. This is designated as the bond distance of the two atoms.

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