1. Name this piece of lab equipment

Question 1 of 17

2. A sample of carbon contained 98.90% carbon-12 and 1.10% carbon-13. Calculate the relative atomic mass of carbon

Question 2 of 17

3. Assuming bond energies in kJ/mol: H-C 412, C-C 348, O-H 463, C-O 360, C=C 612. Calculate the molar enthalpy change for the reaction: ethanol → ethene + water

Question 3 of 17

4. What is meant by the term molecular formula?

Question 4 of 17

5. What volume does 0.5 moles of ethene gas occupy (at rtp)

Question 5 of 17

6. State the steps for calculating empirical formula

Question 6 of 17

7. Complete the following expression: Mᵣ =

Question 7 of 17

8. What is the meaning of the word mole in Chemistry?

Question 8 of 17

9. Use Q=mcΔT and c=4.18J/°C/g. A spatula of sodium fluoride is put into a boiling tube with 25cm³ of water. The temperature drops from 22.0°C to 18.6°C. What is the total heat energy change?

Question 9 of 17

10. What mass of calcium bromide will fully react with 71g of chlorine?

Question 10 of 17

11. Calculate the relative formula mass(Mr) of a molecule of bromine (Br₂)

Question 11 of 17

12. A beaker of 2 dm³ of ammonium nitrate solution contains 1 mol of ammonium nitrate. What is the concentration of the solution?

Question 12 of 17

13. In a combustion calorimetry experiment, 0.78g of ethanol (C₂H₅OH) produced 12,540 J of heat energy. Calculate the molar enthalpy change.

Question 13 of 17

14. State the expression for calculating % yield.

Question 14 of 17

15. To determine the formula of a metal oxide by combustion, magnesium is heated in a crucible. Why is a lid lifted from time to time?

Question 15 of 17

16. A graph shows the solubility of sodium chloride in water at 50°C is 34g/100g. At that temperature, what mass of sodium chloride will dissolve in 50g water?

Question 16 of 17

17. An oxide of nitrogen contains 26% nitrogen and 74% oxygen and has a relative molecular mass of 108. Find the empirical and molecular formulae for the oxide.

Question 17 of 17