Compound A is an organic compound which contains Carbon, Hydrogen and Oxygen. When 0.240g of the vapour of A is slowly passed over a large quantity of heated Copper (II) oxide, CuO, the compound A is completely oxidized to carbon dioxide and water. Copper is the only other product of the reaction. The products are collected and it is found that 0.352g of CO2 and 0.144g of H2O are formed. Questions : 1) Calculate the mass of carbon present in 0.352g of CO22) Use this value to calculate the amount in moles of carbon atoms present in 0.240g of A

1) 0.009 61 g C; 2) 0.008 00 mol C

Step-by-step explanation:

You know that you will need a balanced equation with masses, moles, and molar masses, so gather all the information in one place.

M_r: 12.01 44.01

C + ½O₂ ⟶ CO₂

m/g: 0.352

1) Mass of C

Convert grams of CO₂ to grams of C

44.01 g CO₂ = 12.01 g C

Mass of C = 0.352 g CO₂ * 12.01 g C/44.01 g CO₂

Mass of C = 0.009 61 g C

2) Moles of C

Convert mass of C to moles of C.

1 mol C = 12.01 g C

Moles of C = 0.00961 g C * (1 mol C/12.01 g C)

Moles of C = 0.008 00 mol C

All the carbon comes from Compound A, so there are 0.008 00 mol C in Compound A.