Please I need your help When zinc metal reacts with oxygen gas, 2Zn(s) + O2(g) → 2ZnO(g), large amounts of light and heat are released. A student states that this reaction is a combustion reaction but not a redox reaction. Do you agree? Defend your answer by explaining whether or not it meets the requirements of each type of reaction.

Every redox reaction equation contains two or more atoms (usually from different elements) changing their oxidation state (number) through a transfer of one or more electrons. The simultaneous processes of oxidation and reduction are exactly balanced, such that electrons do not appear in the overall equation. You can assign oxidation states to atoms on their own or in chemical compounds based on certain rules.

To confirm that this is a redox reaction, we must assign oxidation...

1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles