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3 years ago

A student measures the mass of a sample as 9.67g. Calculate the percentage error, given that the correct mass is 9.82

Chemistry

2 answers:

max2010maxim [7]3 years ago

8 0

Answer:

1.5 %

Explanation:

Given data:

Theoretical value = 9.67 g

Actual value = 9.82 g

Percentage error = ?

Solution:

Formula

<em>percentage error = (Theoretical value - actual value / actual value) ×100</em>

percentage error = 9.67 - 9.82 /9.82 ×100

percentage error = -0.15/ 9.82 ×100

percentage error = -0.015×100

percentage error = 1.5 %

pishuonlain [190]3 years ago

5 0

<h3>Answer:</h3>

1.53%

<h3>Explanation:</h3>

We are given;

Experimental value as 9.67 g

Actual measurement as 9.82 g

We are required to calculate the percentage error;

Percentage error is given by dividing the absolute value of the difference between the experiment value and the actual value then dividing by the actual value and multiplying by 100.
That is;

% error = ((Experimental value -Actual value)÷ Actual value) × 100%

Difference between experimental value and actual value = 9.67 g - 9.82 g

= -0.15

Therefore, Absolute value = 0.15

Therefore;

% error = (0.15 ÷ 9.82 g) × 100

= 1.527%

= 1.53%

Thus, the percentage error is 1.53%

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3 years ago

There are three naturally occurring isotopes of the hypothetical element hilarium 45Hi, 46Hi, and 48Hi. The percentages of these

den301095 [7]

Answer:

46.761g/mol

Explanation:

Given parameters:

Element = Hilarium , Hi

Isotopes: Hi- 45, Hi-46 and Hi- 48

Natural abundance of Hi-45 = 18.3%

Hi-46 = 34.5%

Hi-48 = 47.2%

Unknown:

Atomic weight of naturally occurring Hilarium = ?

Solution:

Isotopes have been studied extensively by mass spectrometry. The method is used to determine the proportion/percentage/fraction by which each of the isotopes of an element occurs in nature. The proportion is called geonormal abundance. From this we can calculate the atomic weight of an element.

We can use the expression below to find this value:

Atomic weight = m₄₅α₄₅ + m₄₆α₄₆ + m₄₈α₄₈

m is the atomic mass of each isotope and α is the abundance

Atomic weight = (45 x $\frac{18.3}{100}$ ) + (46 x $\frac{34.5}{100}$ ) + (48 x $\frac{47.2}{100}$ )