I can not determine the answer for this problem...can someone please help me?
Determine the number if moles of MgO that form from the reaction of 4.4 moles of O2 in the following unbalanced reaction:
Mg + O2 ----> MgO
The balanced equation is:
2Mg + O2 -----> 2MgO
a. 1.1 moles
b. 4.4 moles
c. 17.6 moles
d. 2.2 moles
e. 8.8 moles
If I did this right I get 8.8 moles, is that correct or I am still doing this wrong? Please Help me!
you are correct. You get twice the moles of product as you had of O2
To determine the number of moles of MgO that form from the reaction, you need to use the stoichiometry of the balanced equation.
The balanced equation is: 2Mg + O2 -----> 2MgO
From the balanced equation, you can see that for every 2 moles of MgO formed, there are 1 mole of O2 consumed. Therefore, the ratio of moles of O2 to moles of MgO is 1:2.
You are given that there are 4.4 moles of O2, so you can set up a proportion to find the number of moles of MgO:
(4.4 moles O2 / 1) x (2 moles MgO / 1 mole O2) = 8.8 moles MgO
So, the correct answer is e. 8.8 moles.
Therefore, your calculation is correct! Well done!