A small flask and stopper is found to weigh 23.994 g. It is carefully filled with water and reweighed. The new weight is 50.00 g. If the water density is taken as 1.000 g/ml, what is the volume of the flask?

Calculate the density of a liquid in g/mL to the correct number of significant digits, if a flask containing 9.55 mL of the liquid weighs 157.2 g with the liquid and 148.4 g when empty.

A backyard swimming pool holds 185 cubic yards (yd³) of water. What is the mass of the water in pounds?

A block of solid that weighs 58.16 g was placed in a container with a 100 mL capacity. It was then filled to capacity with liquid benzene and measured to have a combined weight of 96.15 g. Calculate the density of the solid if the density of benzene is 0.879 g/mL.

A student performs an experiment to determine the density of a sugar solution. She obtains the following results: 1.70 g/mL, 1.75 g/mL, 1.66 g/mL, and 1.68 g/mL. How should she report the average density of her measurements, including the uncertainty?

Calculate the temperature in °C of nitrogen gas (N2) with a density of 2.28 kg/m³ at a pressure of 2 atm. (Assume ideal gas behavior and use R = 0.0821 L·atm/mol·K for calculations.)

Calculate the number of atoms in a copper rod with a length of 9.85 cm and a radius of 1.05 cm. The density of copper is 8.96 g/cm³. (The volume of a cylinder is V = πr²l.) Express the number of atoms to three significant figures. Assume the molar mass of copper is 63.55 g/mol and Avogadro's number is 6.022 × 10²³ atoms/mol.

Greg has a blood volume of 5.9 qt. If the density of blood is 1.06 g/mL, what is the mass, in grams, of Greg's blood? (Note: 1 qt = 946.353 mL)