Balancing Equations Coefficient Question

[Amanda Bueno-Kling]

Sometimes when I am balancing chemical equations, I end up with coefficients that are not whole numbers. For example, there are 15 mols of O on one side, and on the other side I have to add a coefficient before O2. I can't put 7.5, even though 7.5 * 2 = 15, because I know coefficients have to be whole numbers. Is the best thing to do in this case multiply every coefficient in the reaction by 2? This should preserve the ratio while making everything a whole number?

[Hannah Alltucker 3L]

Yes, you would multiply the equation by two in order to make all coefficients whole numbers. Having whole number coefficients makes the equation easier overall to use in future steps.

[Andreas Krumbein 1L]

Yes, you can't have a half of an atom (unless you want to experience dire consequences), and so in a molecular equation you should scale each coefficient up to the lowest whole number. (eg, 7.5 should become 15, and 2.75 should become 11). If at any point if you write a fraction as a coefficient in a molecular equation, it will be marked wrong.

[Erika Sosa-Cruz 1J]

Yes the best thing to do would be to multiply the coefficients by two because we want whole numbers, and to answer your second question it will in fact preserve the ratio.

[Kelly Tran 1J]

Yes, you would multiply each coefficient by 2 since the stoichiometric coefficients must be whole numbers. In the notes for this topic, Dr. Lavelle stated how multiplying both sides of the chemical equation by a number does not affect the balance of each atom type.

[Jaclyn Schwartz 1I]

Yes, that is exactly right! Using fractions and non-whole numbers makes it more difficult to solve. And when you multiply by 2 on each side, it does not unbalance the equation because you are doing it to both sides.

[Andrew Yoon 3L]

If your equation has any stoichiometric coefficients that are fractions, you need to convert them to whole numbers. Since you can't have a fraction of a compound, you need to multiply whatever number on one side to the other as well in order for it to be balanced.

[John_Tran_3J]

To correctly balance an equation with fractions as stoichiometric coefficients, you must multiply every coefficient with the demoniator of the fraction. This action causes every coefficient (including the faction) to become a whole number.

[Sukhkiran Kaur 3I]

Yes that's right, since you would use the lowest value possible that would give you whole numbers for coefficients.

[abby hyman]

Yes, you have the right idea about it. since you do not want a coefficient to be 15/2 you have to multiply every coefficient by 2 so they are all in whole numbers and maintain the correct ratio

[Sreeram Kurada 3H]

Yeah I would continue doing the same thing you are doing right now since it is much easier to balance the chemical equation.

[Michelle Nguyen 3F]

When that happens, try to multiply it to get the lowest coefficient possible. For instance, if you have 7.5, multiply it by 2 to get 15. If you have 3.33, multiply by 3 to get 10. It's important to look at the decimals to see what number you should multiply by.

[Susan Chamling 1F]

Yes, you would want to multiply your coefficients by the same number in order to get whole ratios. As long as you preserve the ratio, multiplying the coefficients is fine.

[Annette Fishman]

Yes, you should multiply your coefficients by the same number in order to get whole ratios. That number should be the smallest coefficient possible, or you'll need to simplify. For example, if the coefficient is 1.5, you'd want to multiply by 2. If 3.33, multiply by 3. When you put it in fraction for it's easier to see - 3/2 *2 = 3. Don't forget to preserve the ratio of the reactants and products, and you'll be good :)

[Gicelle Rubin 1E]

As everyone has said, as long as you multiply both by the same number, you should be fine! :)

[Bai Rong Lin 2K]

Sometimes when I am balancing chemical equations, I end up with coefficients that are not whole numbers. For example, there are 15 mols of O on one side, and on the other side I have to add a coefficient before O2. I can't put 7.5, even though 7.5 * 2 = 15, because I know coefficients have to be whole numbers. Is the best thing to do in this case multiply every coefficient in the reaction by 2? This should preserve the ratio while making everything a whole number?

you just multiply the coefficient by to in order to reach a whole number for the final balance equation.

[April Pazos 3D]

Yes, in order to eliminate the fraction, multiply by the whole number it is divided by to have only whole numbers as stochiometric coefficients.

[Leah Wildmann 1F]

Yes, the best thing to do is to multiply both sides of the equation by the denominator in the stoichiometric coefficient that is a fraction. This will make all the coefficients whole numbers, which will make calculations much easier.

[Joellen 1B]

Hey! So I would write it out as a fraction first. For example, if you have a coefficient of 7.5, I would write out 15/2. And then to get rid of that fraction, I would multiply 15/2 as well as all of the other coefficients by 2 as well so that they are all still the same ratio.

[Isabelle Rieke-Wey 2G]

Hi!
I would write 7.5 out as a fraction (so 15/2). Then I would multiply all of the coefficients in the chemical equation by 2 to clear out the fraction, and have only whole numbers. Then the equation should be balanced! Hope thats helps

[105784203]

Sometimes when I am balancing chemical equations, I end up with coefficients that are not whole numbers. For example, there are 15 mols of O on one side, and on the other side I have to add a coefficient before O2. I can't put 7.5, even though 7.5 * 2 = 15, because I know coefficients have to be whole numbers. Is the best thing to do in this case multiply every coefficient in the reaction by 2? This should preserve the ratio while making everything a whole number?

Yes, that is the whole point of using fraction stoich coefficients, you multiply out the denominator in order to get whole coefficients.

[Anish_Marripati_2F]

Yes, if the coefficient is not a whole number then you need to multiply. In your question, you stated 7.5. You are correct in the fact that you have to multiply the rest of the equation by 2 to get the blanked chemical equation.

[Do Yeun Park]

Yes, you would need to multiply the entire stoichiometric coefficients by 2 in order to get whole number.

[Jennifer Kainth 3L]

Hi,
You're absolutely correct! Multiplying by 2 would cause all coefficients to become whole numbers. Overall, it is much easier to interpret an equation if the coefficients are whole numbers.
Hope that helps!

[Mya_Chiarappa_2C]

Yes! All coefficients should be the lowest possible whole numbers, so you should multiply by whatever number would give you this result.