how many moles of oxygen are needed to react with 3.5moles of ethylene, considering the combustion of ethylen C2 H4 + 3O2 -- 2CO2 + 2H2 O
how would i solve this question what would be the steps
the equation is balanced. so you do:
3.5 moles C2H4 * 3 moles O2 / 1 mole C2H4 = 10.5 moles O2
this part means that 3 moles O2 is over 1 mole C2H4 if that wasn't clear.
thank you
To solve this question, you will need to use the stoichiometric coefficients in the balanced chemical equation. Here are the steps you can follow:
1. Write down the balanced chemical equation:
C2H4 + 3O2 → 2CO2 + 2H2O
2. Identify the mole ratio between ethylene (C2H4) and oxygen (O2) from the balanced equation. In this case, for every 1 mole of ethylene, we need 3 moles of oxygen.
3. Determine the number of moles of oxygen needed to react with 3.5 moles of ethylene.
You can use the mole ratio from step 2 to calculate this. Since the mole ratio is 1 ethylene to 3 oxygen, you can set up a proportion:
1 ethylene / 3.5 ethylene = x oxygen / 1 oxygen
Simplifying the equation, we see that x = (3/1) * 3.5
x = 10.5
So, 10.5 moles of oxygen are needed to react with 3.5 moles of ethylene.
Note: Make sure to always use the balanced chemical equation and the stoichiometric coefficients to determine the mole ratios.