Chemistry Answers

An oxide of nitrogen contains 63.1% oxygen and has a molar mass of 76.0 g/mol.

a. What is the empirical formula of the compound?

b. What is the molecular formula of the compound?

Calculate the molality of solution containing 240.5g of NH4NO3 (ammonium nitrate) dissolved in 1050.0g of water?

An organic compound is known to be nonvolatile and non electrolyte. A 0.35g sample is dissolved in water and diluted to 150mL. The osmotic pressure is measured as 0.04 atm at 250C. The approximate mass number for this compound is 1400g/mol. From the data provided in this problem and knowing that the density Of the solution is 1.00g/mL

a. Calculate the freezing point of the solutions.

b. Determine if the freezing point change would be a good way to determine the molecular mass of the compound.

c. Would the boiling point change be a better determining factor than the freezing point change?

Ethylene glycol C2H6, is a common automobile antifreeze agent. Calculate the freezing point of solution containing 651 grams of EG in 2505 grams of water. The molar mass of EG is 62.01 g/mol (Kf=1.86° C/m) and (Kb= 0.52 ° C/m for water)

Show your solution.

find the percent by volume of a 37 ml solution if it contains 16 ml of potassiuk hydroxide

6.80 g of soduim chloride are added to 265 g of water. find the mole fraction of thesoduim chloride and water in the solutiom

Calculate the boiling point of solution containing 3.5 g sugar (molar mass=342g) dissolve in water. Show your solution.

For a solution of pH 5.0 at 25°C, calculate [H⁺] and [OH^-].

The presence of SO² in the atmosphere causes acid rain. What percentage of sulfur is present in S0²(Molar mass=64.07 g/mole)?

How many atoms of gold are there in 7g of a karat gold ring?