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GREYUIT [131]
3 years ago
12

A naturally occurring sample of an element contains only two isotopes. The first isotope has a mass of 68.9255 amu and a natural

abundance of 60.11%. The second isotope has a mass of 70.9247 amu. Find the atomic mass of the element.
Chemistry
1 answer:
Ket [755]3 years ago
3 0

Answer:- The average atomic mass or the atomic mass of the element is 69.7230 amu.

Solution:- The atomic mass or also known as average atomic mass of an element is calculated from it's isotopes by using the formula:

average atomic mass = mass of First isotope(abundance) + mass of second isotope(abundance)

From given data, the mass of first isotope is 68.9255 amu and mass of second isotope is 70.9247 amu. percent abundance for the first isotope is 60.11%. The sum of percent abundance of all the isotopes of an element is always 100. So, the percent abundance of second isotope = 100 - 60.11 = 39.89%

We convert the percent abundances to the decimals and then plug in the values in the formula to calculate the average atomic mass.

First isotope abundance = 0.6011

second isotope abundance = 0.3989

average atomic mass = 68.9255(0.6011) + 70.9247(0.3989)

average atomic mass = 41.4311 + 28.2919

average atomic mass = 69.7230 amu

So, the average atomic mass or the atomic mass of the element is 69.7230 amu.

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The acetylene tank contains 35.0 mol C2H2, and the oxygen tank contains 84.0 mol O2.
harkovskaia [24]

Answer:- As per the question is asked, 35.0 moles of acetylene gives 70 moles of carbon dioxide but if we solve the problem using the limiting reactant which is oxygen then 67.2 moles of carbon dioxide will form.

Solution:- The balanced equation for the combustion of acetylene is:

2C_2H_2(g)+5O_2(g)\rightarrow 4CO_2(g)+2H_2O(g)

From the balanced equation, two moles of acetylene gives four moles of carbon dioxide. Using dimensional analysis we could show the calculations for the formation of carbon dioxide by the combustion of 35.0 moles of acetylene.

35.0molC_2H_2(\frac{4molCO_2}{2molC_2H_2})

= 70molCO_2

The next part is, how we choose 35.0 moles of acetylene and not 84.0 moles of oxygen.

From balanced equation, there is 2:5 mol ratio between acetylene and oxygen. Let's calculate the moles of oxygen required to react completely with 35.0 moles of acetylene.

35.0molC_2H_2(\frac{5molO_2}{2molC_2H_2})

= 87.5molO_2

Calculations shows that 87.5 moles of oxygen are required to react completely with 35.0 moles of acetylene. Since only 84.0 moles of oxygen are available, the limiting reactant is oxygen, so 35.0 moles of acetylene will not react completely as it is excess reactant.

So, the theoretical yield should be calculated using 84.0 moles of oxygen as:

84.0molO_2(\frac{4molO_2}{5molO_2})

= 67.2molCO_2

7 0
3 years ago
Read 2 more answers
First answer will be brainliest!!
igomit [66]
I think it is rarefaction. But im not sure

8 0
3 years ago
Which substance produces hydroxide ions in solution?
Olegator [25]

Answer:

An Arrhenius Base

Explanation:

The definition of this is a base that is a hydroxide ion donor.

8 0
2 years ago
Which two compounds are classified as bases by the Brønsted-Lowry definition, but not by the Arrhenius definition, and why?
konstantin123 [22]

Answer: Ammonia (NH3) and sodium carbonate (Na2CO3), because they accept hydrogen ions but lack hydroxide ions.

Explanation:

i took the test and got it correct :) hope this helps

6 0
3 years ago
How many hydrogen atoms are in 5 molecules of isopropyl alcohol
pychu [463]
You have to double them
5 0
3 years ago
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