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How do you balance #P_4 + O_2 -> 2P_2O_3#?

Answer 1

Verify that there are the same number of atoms on both sides by counting the atoms on each side.

On the left side (or left of arrow), P = 1 #xx# 4 = 4 atoms of P O = 1 #xx# 2 = 2 atoms of O

On the right side P = 2 #xx# 2 = 4 atoms of P O = 2 #xx# 3 = 6 atoms of O

O is not balanced, but P is.

Find the lowest common multiple (LCM) of number of atoms present in O. The LCM between 2 and 6 is 6. On the left hand side, we need to make the number of atoms of O from 2 to become 6 by multiplying 3. So insert a 3 in front of #O_2# therefore its composed of 6 atoms.

Check your equation now: #P_4 + 3O_2 => 2P_2O_3#

Now, confirm that there are the same number of atoms on both sides by double checking. - IMPORTANT

P = 4 atoms left and 4 atoms right; this is a balanced array; O = 6 atoms left and 6 atoms right; this is a balanced array.

You can now write your balanced equation if they are all balanced.

Overall, your balanced equation should look like: #P_4 + 3O_2 => 2P_2O_3#

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Answer 2

Cooper Adams

Balanced equation: P4 + 5O2 → P4O10

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

How do you balance #P_4 + O_2 -&gt; 2P_2O_3#?

How do you balance #P_4 + O_2 -> 2P_2O_3#?