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3 cards from this section. Quick, good the night before a test.
Calculate the percentage uncertainty for a mass of 50.0 g measured with an uncertainty of ± 0.5 g.
Divide the uncertainty by the measured value and multiply by 100.
If the length of an object is measured as 20.0 cm with an uncertainty of 0.1 cm, what is the percentage uncertainty?
Apply the same formula as above.
What do you do with the percentage uncertainties when multiplying or dividing two values?
Remember the rule of uncertainty propagation.
True or False: Absolute uncertainty is always more informative than percentage uncertainty.
Consider what each value represents.
A student measures a mass of a chemical as 12.5 g with a ± 0.2 g uncertainty and a volumetric reading of 4.00 mL with a ± 0.01 mL uncertainty. How do they report the density of the chemical with its uncertainty?
Remember to convert the uncertainty into absolute values for final reporting.
If the concentration of a solution is measured at 0.0500 M with a 0.0010 M uncertainty, and it's diluted by transferring to 200 mL while maintaining that uncertainty. What is the final concentration and its uncertainty?
Consider dilution effects on concentration and how the uncertainties apply directly.
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