Suppose you were calibrating a 50.0 ml volumetric flask using distilled water. the flask temperature was at 20°c, and you assume
d that the distilled water was as well. however, you later discover that the actual water temperature was 14°c instead. how is the mass of the 50.0 ml of distilled water you measured at 14°c different from the mass of 50.0 ml of distilled water at 20°c?
Density is sensitive to temperature for gases and liquids, although not much for liquids. We use the data in the picture. Using linear interpolation, we determine the densities at 14°C and 20°C.
@20°C: Density = 0.99823 g/cm³ or g/mL @14°C: (10 - 14)/(10 - 20) = (0.99973 - Density)/(0.99973 - 0.99823) Solving for density: Density = 0.99913 g/cm³ or g/mL
Mass @ 20°C = 50 mL * 0.99823 g/mL = 49.9115 g Mass @ 14°C = 50 mL * 0.99913 g/mL = 49.9565 g Difference of Masses = |49.9115 g - 49.9565 g| = 0.045 g
The right answer for the question that is being asked and shown above is that: "B. observed wavelength of light" Planck's constant relates the Joules of energy absorbed/released by matter to the <span>B. observed wavelength of light</span>
The half-life of Plutonium 239 (Pu 239) is 24,100 years.
Explanation:
Half-life is the time required for a quantity to reduce to half of its initial value. This means that in 241000 years, 100g of Pu 239 would be reduced to 50g.