Fractions as Coefficients

[Jack Van Ryan 1A]

Is it possible to have fractions as coefficients when balancing chemical reactions? I came across a problem where I had 2/3 as a coefficient, and I wasn't sure as to whether that's acceptable or not?

Thank you!

[Reza Hemmati 3L]

Hi!

When you come across fractional coefficients in balancing, it's preferred to multiply every coefficient by the number in the denominator(in your case, 3) so that there are no fractional coefficients. This most usually happens with oxygen in combustion reactions, where sometimes you have to double every coefficient because oxygen has a fractional coefficient.

Hope this helps ^^

[Sanjana Sivakumar 2E]

Hello!

I believe if we have fraction as a coefficient, we need to multiply every coefficient by a denominator to create whole numbers.

Hope this helps!

[Jericho Ansay 1C]

Yes, it's possible to have fractions as coefficients, but you would just need to multiply that fraction out so that you get whole numbers. The result would be the final acceptable answer in a balanced chemical equation.

[Vashe Sundar 3H]

Yes, it's possible to have fractions as coefficients! However, it's preferred that you have whole numbers as coefficients. At that point, you will have to convert the fractions into whole numbers by finding the common denominator and multiplying it out.

[Genelle Marcelino-Searles 2G]

Yes, just multiply the coefficients until you get a whole number.

[605778346]

When you have fractions as coefficients, you have to multiply the entire equation so that all coefficients are whole numbers.

[Aaron Martinez]

You can't really have a fraction as a coefficient. If you end up with one, you have to multiply every coefficient in the equation by the least common multiple of all the denominators to get the lowest possible whole number for the coefficients.

[Jessica Ghiuzelian 1H]

Hi! Fractions as coefficients are not really possible, so it is best to convert the fraction to a whole number by multiplying the fraction by the number in the denominator. Remember to multiply all the coefficients in the equation as well since you have to increase all the ratios to keep the equation balanced.

[Kayla Ziebell 1H]

Is it possible to have fractions as coefficients when balancing chemical reactions? I came across a problem where I had 2/3 as a coefficient, and I wasn't sure as to whether that's acceptable or not?

Thank you!

Hi! I would multiple the whole reaction by the denominator, in this case, 3. It would make all the coefficients integers which would make it easier if wanting to do more with the equation.

[Jaipal Virdi 2I]

Typically in balancing equations, you would want to get rid of the the fractions. As others have explained, you can accomplish this by multiplying the whole equation by the denominator of the fraction of the given molecule.

[Sonia Virk 2A]

Fractions as coefficients are usually not acceptable so just multiply the all the coefficients by the denominator of the fractional coefficient so they are all whole numbers. Hope this helps!

[Ryan Lafferty 1L]

We must have whole numbers as our stoichiometric coefficients, so I'd find a common denominator and multiply to get whole numbers.

[Palig Kechichian 3F]

Hi! If you end up getting a fraction, you'd probably have to multiply all the coefficients by the denominator so that you get a whole number and maintain your balanced reaction

[Kelly_Luong_1F]

In balanced equations, you would typically want a whole number as the coefficient so if you do have a fraction as a coefficient, multiplying by a value that will give you all whole number coefficients.

[005502505]

Hi!

When coefficients are fractions, multiplying the bottom of the fraction through to every coefficient is helpful to achieve whole numbers (assuming that all of the other coefficients may be divided by the denominator in the fractional coefficient). Hope this helps!!