Question

What would the product be? for A and B?Item A.

Answer 1

Assuming the reactions are for complete combustion, the products are always carbon dioxide and water, so the unbalanced equation is:

`C_5H_(12)(g)+8O_2\to CO_2(g)+H_2O(g)`

Now, we need to balance it.

As we can see, the carbon atom, C, only appears in one place on both sides, so let's start by balancing it.

We have 5 carbon on the left side, and one carbon of the right side, so we can balance the carbon atom by adding a coefficient of 5 on CO₂:

`C_5H_(12)(g)+8O_2(g)\to5CO_2(g)+H_2O(g)`

Now, we can balance the hydrogen atom, H. We have 12 hydrogen on the left side and 2 per water molecule on the right side. So, we can put the coefficient 6 on the water, so we balance the H atom:

`C_5H_(12)(g)+8O_2(g)\to5CO_2(g)+6H_2O(g)`

Now, we need to check wheter the oxygen atom, O, is balanced.

On the left side, we have 8 times 2, so 16 oxygen.

On the right side we have 5 times 2 on CO₂, so 10, plus 6 on the water, so a total of 16 oxygen.

Since both side are equal, the equation is balanced.

So, the final equation is:

`C_5H_(12)(g)+8O_2(g)\to5CO_2(g)+6H_2O(g)`