given the balanced equation:
2Al2O3(s)-->4Al(s)+302(g)
What is the total number of moles of O2 that are produced when 8.0 mol of Al2O3(s)are totally decomposed ?
please help me.
2Al2O3(s)-->4Al(s)+302(g)
From the equation 2 moles of Al2O3 yields 3 moles of O2
so
From the equation 4 moles of Al2O3 yields 6 moles of O2
so
From the equation 8 moles of Al2O3 yields ?? moles of O2
so the answer is 2 moles ?
i meant 12* moles
wait is it 24 moles ?
It's 12 moles. Cross multiply 8x6= 48, and then 48/4= 12
To find the total number of moles of O2 produced when 8.0 mol of Al2O3(s) is decomposed, you need to use the stoichiometry of the balanced equation.
From the balanced equation:
2Al2O3(s) → 4Al(s) + 3O2(g)
It shows that for every 2 moles of Al2O3(s) decomposed, you get 3 moles of O2(g) produced.
So, you can set up a proportion using this information:
2 mol Al2O3 : 3 mol O2 = 8.0 mol Al2O3 : x
To solve for x (the number of moles of O2 produced), you cross-multiply and solve for x:
(2 mol Al2O3 / 3 mol O2) * 8.0 mol Al2O3 = 5.33 mol O2
Therefore, when 8.0 mol of Al2O3 is completely decomposed, 5.33 moles of O2 are produced.