The noble gas argon was discovered by Sir Walter Ramsay and John William Strutt in England in 1895.  Through this discovery, they made highly accurate measurements of gas densities.  Their experimentally determined densities are:        Oxygen                1.42952 g/L Nitrogen              1.25718 g/L Air                          1.29327 g/L 1) To determine the density of atmospheric nitrogen, Strutt removed the oxygen, water, carbon dioxide, and argon from air and then filled an evacuated glass tube with the remaining gas.   He determined that a mass of 0.20389 g of nitrogen has a density of 1.25718 g/L under standard conditions of temperature and pressure.  What is the volume of the glass tube in cm3?

A chemist prepares a solution of potassium chloride (KCI) by measuring out 93.7 mg of KCl into a 300. mL volumetric flask and filling to the mark with distilled water. Calculate the molarity of CI anions in the chemist's solution. Be sure your answer is rounded to 3 significant digits. 0 mol L

A geochemist measures the concentration of salt dissolved in Lake Parsons and finds a concentration of 69.32 g.L The geochemist also measures the concentration of salt in several nearby non-isolated lakes, and finds an average concentration of 5.02 g⋅L¯¹. Assuming the salt concentration in Lake Parsons before it became isolated was equal to the average salt concentration in nearby non-isolated lakes, calculate the percentage of Lake Parsons which has evaporated since it became isolated. Be sure your answer has the correct number of significant digits.

Suppose 1.47 g of zinc iodide is dissolved in 100. mL of a 76.0m M aqueous solution of potassium carbonate. Calculate the final molarity of zinc cation in the solution. You can assume the volume of the solution doesn't change when the zinc iodide is dissolved in it. Be sure your answer has the correct number of significant digits.

A chemistry student must write down in her lab notebook the concentration of a solution of potassium chloride. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: • The label on the graduated cylinder says: empty weight: 1.55 g • She put some solid potassium chloride into the graduated cylinder and weighed it. With the potassium chloride added, the cylinder weighed 31.436 g. • She added water to the graduated cylinder and dissolved the potassium chloride completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 166.4 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. -1 g.mL x10 × Ś

What is the molar volume of solid quartz, SiO2?(density =2.65g/cm3) (molar volume is the volume occupied by one mole)

Aqueous hydrobromic acid  HBr  will react with solid sodium hydroxide  NaOH  to produce aqueous sodium bromide  NaBr  and liquid water  H2O . Suppose 34.8 g of hydrobromic acid is mixed with 13. g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

Suppose 5.71 g of potassium chloride is dissolved in 350. mL of a 64.0 m M aqueous solution of silver nitrate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the potassium chloride is dissolved in it. Be sure your answer has the correct number of significant digits.

11. Radon gas produces radioactive particles and in high concentrations can result in lung cancer in humans. The radon gas level inside a basement is measured at 4.5 × 10ª Curies/cm³. How many picoCuries of radon are present in the room if the room's dimensions are 7.2 m × 8.5 m × 4.0 m?

A chemist prepares a solution of nickel(II) chloride NiCl2 by measuring out 97.μmol of nickel(II) chloride into a 150.mL volumetric flask and filling the flask to the mark with water. Calculate the concentration in mmol/L of the chemist's nickel(II) chloride solution. Round your answer to 2 significant digits.