Calculator Inputs
Example Data Table
This example uses mass based input values for a six element sample.
| Element | Atomic Weight (g/mol) | Sample Amount (g) | Interpretation |
|---|---|---|---|
| O | 15.999 | 46.60 | Major light element contribution. |
| Si | 28.085 | 27.70 | Strong structural component. |
| Al | 26.982 | 8.10 | Moderate abundance contribution. |
| Fe | 55.845 | 5.00 | Heavy element, lower mole share. |
| Ca | 40.078 | 3.60 | Secondary composition driver. |
| Mg | 24.305 | 2.10 | Minor but meaningful presence. |
Formula Used
1. Convert measured input to moles.
For mass based input: ni = mi / Ai
For mole based input: mi = ni × Ai
2. Find atomic fraction.
xi = ni / Σn
3. Convert atomic fraction to atomic percent.
Atomic % = xi × 100
4. Find weight fraction.
wi = mi / Σm
5. Convert weight fraction to weight percent.
Weight % = wi × 100
6. Convert weight fraction to ppm.
PPM = wi × 1,000,000
7. Normalize abundance to any total.
Normalized abundance = xi × N, where N is the chosen normalization target.
8. Estimate empirical ratio.
Empirical ratio = ni / min(n)
How to Use This Calculator
- Select whether your measured data is mass based or mole based.
- Choose the matching input unit for every amount entered.
- Enter each element symbol, atomic weight, and measured value.
- Choose a normalization mode for ratios or scaled abundance reporting.
- Select the chart metric you want to visualize with Plotly.
- Press the calculate button to show the summary above the form.
- Review the table for atomic percent, weight percent, ppm, and empirical ratio.
- Use the export buttons to save the result table as CSV or PDF.
FAQs
1. What does elemental abundance mean here?
It represents each element’s share within the sample. The calculator reports abundance as atomic percent, weight percent, ppm, normalized units, and relative dominance.
2. Should I enter mass or moles?
Use the basis that matches your laboratory measurement. Mass input suits weighed samples, while mole input suits already converted stoichiometric or spectrometric datasets.
3. Why is atomic weight required?
Atomic weight connects mass and moles. Without it, the calculator cannot convert between physical mass share and atomic share correctly.
4. What is normalized abundance?
Normalized abundance rescales atomic fraction to a chosen total, such as 1, 100, or 1,000,000. This helps match reporting standards or compare datasets consistently.
5. Can I use isotopic atomic masses?
Yes. When you need isotope specific work, enter the exact isotopic mass. That makes conversions more consistent with your analytical assumptions.
6. Why are empirical ratios not whole numbers?
The ratio is a direct mole comparison. Experimental data often produces decimals before rounding to a likely formula pattern or stoichiometric approximation.
7. What does ppm by mass show?
PPM expresses each element’s mass fraction on a one million unit basis. It is useful for trace analysis, impurity screening, and contamination reporting.
8. Can I compare two samples with this page?
Yes. Run one sample, export it, then calculate the second sample. The normalized outputs and Plotly chart make side by side review easier.