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Vikentia [17]
3 years ago
12

Naturally occurring gallium is a mixture of isotopes that contains 60.11% of Ga-69 (atomic mass = 68.93 u) and 39.89% of Ga-71 (

atomic mass = 70.92 u). Which numerical setup can be used to determine the atomic mass of naturally occurring gallium?
Mathematics
2 answers:
VladimirAG [237]3 years ago
7 0

Answer:

69.724

Step-by-step explanation:

You have to assume that you have 10000 atoms of  gallium which would mean that 6011 of those atoms weigh 68.93 u while 3989 atoms weighs 70.92 u. So to calculate this calculation can be set up this way.

RAM =\frac{6011*68.93+3989*70.92}{10000} = 69.724

Stels [109]3 years ago
4 0

Answer:

69.72 u

Step-by-step explanation:

To find the relative atomic mass you multiply the percentage of occurrence by the mass of occurrence and add them up, then you divide by 100.

((60.11 × 68.93) + (39.89 × 70.92)) ÷ 100

=69.723811

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Answer:

40.625%

Step-by-step explanation:

This is a very simple question.

We have to understand converting word equations to algebraic ones.

"is" means "="

"of" means "*"

So, we can write:

39 = what percent * 96

Now, we let "what percent" be "p" and solve the equation for p:

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Step-by-step explanation:

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