Indium has two naturally occurring isotopes and an atomic mass of 114.818 amu. In- 113 has a mass of 112.904 amu and an abundance of 4.3%. What is the identity and percent abundance of indium's other isotope. I am very confused on how do I set up this conversion problem?

atomic masses are weighted averages of all of the isotopes.

% in 113 = 4.3% and since the isotopes must add to 100%, then 100 - 4.3 = 95.7% for the other isotope.
Let x = to mass of the other isotope. Then set up the average.

112.904(0.043) + (x)(0.957) = 114.818 and solve for x.
95&% is part of the answer. x is the other part of the question. Check my numbers against typos. I make a typo now and then.

5.07301149

To solve this problem, let's define the following:

Let x represent the abundance of the other isotope of indium (which we don't know yet)
Let A represent the atomic mass of the other isotope of indium

We are given the following information:

Isotope Indium-113:
- Mass (112.904 amu)
- Abundance (4.3%)

Isotope Indium-x:
- Mass (unknown)
- Abundance (unknown)

Since indium has two naturally occurring isotopes and the total atomic mass is given as 114.818 amu, we can set up the following equation:

(112.904 amu * 4.3%) + (A * x%) = 114.818 amu

Now, we can solve for A by rearranging the equation:

A * x% = 114.818 amu - (112.904 amu * 4.3%)
A * x% = 114.818 amu - 4.854712 amu
A * x% = 109.963288 amu

To find the value of x, we need to divide both sides of the equation by A:

x% = (109.963288 amu) / A

We don't know the value of A yet, so let's represent it as a constant. We can rename A as a variable, y, for convenience:

x% = (109.963288 amu) / y

Now, let's rearrange the equation to solve for y:

y = (109.963288 amu) / x%

So, the identity and percent abundance of indium's other isotope can be represented as:
- Identity: This isotope is indium-y (the letter y represents an unknown)
- Percent abundance: x% (which we calculated as x% = (109.963288 amu) / y)

Now you can plug in the known values to find the abundance of the other isotope.

To solve this conversion problem, you need to set up an equation using the given information and solve for the abundance of the other isotope of indium.

Let's represent the abundance of the other isotope (unknown) as "x." Therefore, the sum of the abundances of the two isotopes should equal 100%, so we have:

x + 4.3% = 100%

To solve for "x," we can then subtract 4.3% from both sides of the equation:

x = 100% - 4.3%
x = 95.7%

Therefore, the percent abundance of the other isotope of indium is 95.7%.