Michael burns a Metal, X in oxygen. There is a single product, an oxide of the Metal. Given that 25.4 grams of X Burns in 3.2 grams of Oxygen, write a Balanced Equation for this Reaction. Show workings Ar of Metal X: 63.5 Mr of X Oxide: 143.0

1. Find mass of Metal Oxide made. This is the Only Product so this can mean the Mass of the Metal Oxide can be equals to the Total Mass of the Reactants [25.4g+3.4g = 28.6g] 2. Divide the Mass of each Substance by its Ar or Mr [Metal X=25.4 / 63.5 = 0.40m] [O2= 3.2/32=0.10] [X Oxide = 28.6/143 = 0.20] 3. Divide by the number of the Smallest Moles [Here its 0.10] [O.4/0.1=4] [0.10/0.10=1] [0.20/0.10=2.0 4. Numbers are back to Whole Numbers, so you can write now the Balanced Equation [4X + O²= 2X²O] [You get the Oxide because of the Metal X reacting with the Oxygen]