Consider the following reversible reaction.
2 answers:
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Hey there! Hello!
Not sure if you still need the answer to this question, but I'd love to help out if you do.
So, the way to balance this equation is pretty simple. First, you need to keep in mind that molecules of hydrogen and oxygen do not come in single molecules, but in bonded pairs, represented by H2 and O2.
But, that's incorrect. The combination of 2 hydrogen molecules with 1 oxygen molecule yields water, but that leaves one oxygen molecule leftover. When broken down, this is how many of each molecule is on each side of the previously stated equation:
Left:
H: 2
O: 2
Right:
H: 2
O: 1
So we have to multiply H2O on the right side by 2 in order to get this:
Left:
H: 2
O: 2
Right:
H: 4
O: 2
The last step is to multiply H2 on the left by two to make it match up with the right side, balancing the equation:
Left:
H: 4
O: 2
Right:
H: 4
O: 2
That makes our equation balanced! I hope this helped you out, feel free to ask any additional questions if you need further clarification. :-)
Not sure if you still need the answer to this question, but I'd love to help out if you do.
So, the way to balance this equation is pretty simple. First, you need to keep in mind that molecules of hydrogen and oxygen do not come in single molecules, but in bonded pairs, represented by H2 and O2.
But, that's incorrect. The combination of 2 hydrogen molecules with 1 oxygen molecule yields water, but that leaves one oxygen molecule leftover. When broken down, this is how many of each molecule is on each side of the previously stated equation:
Left:
H: 2
O: 2
Right:
H: 2
O: 1
So we have to multiply H2O on the right side by 2 in order to get this:
Left:
H: 2
O: 2
Right:
H: 4
O: 2
The last step is to multiply H2 on the left by two to make it match up with the right side, balancing the equation:
Left:
H: 4
O: 2
Right:
H: 4
O: 2
That makes our equation balanced! I hope this helped you out, feel free to ask any additional questions if you need further clarification. :-)