Barium carbonate decomposes when heated.
BaCO3(s) → BaO(s) + CO2(g)
(a) A student heated a 10.0 g sample of barium carbonate until it was fully decomposed.
(i) Calculate the number of moles of barium carbonate the student used.
moles of barium carbonate =
(ii) Calculate the mass of carbon dioxide gas produced at room temperature and pressure. Give your answer in g.
mass of carbon dioxide =
(b) The student added 2.00 g of the barium oxide produced to water.
BaO + H2O → Ba(OH)2
Calculate the mass of barium hydroxide that can be made from 2.00 g of barium oxide. The Mr of Ba(OH)2 is 171.
mass of barium hydroxide =
(c) A 1.50 g sample of barium hydroxide was dissolved in water. The total volume of the solution was 100 cm3. A 25.0 cm3 portion of the barium hydroxide solution was titrated against hydrochloric acid. The volume of hydrochloric acid required was 18.75 cm3.
Ba(OH)2 + 2HCl → BaCl2 + 2H2O
(i) Calculate how many moles of barium hydroxide were in the 25.0 cm3 portion used in the titration.
moles of barium hydroxide =
Answer:
calculate is the best just vat