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### Percent yield

Posted: Thu Oct 05, 2017 6:26 pm
For M1 the question asks what is the percent yield of hydrazine? The question gives the net ionic equation for the reaction. I was wondering if the net ionic equation plays a role in this problem since some of the dissolved ions are not written.

### Re: Percent yield

Posted: Thu Oct 05, 2017 6:50 pm
You don't need to care about other solutes that are not involved in the reaction since they have no influence on the reaction.
The following steps are what you need to solve the problem:
1. converting 35 g ammonia to moles
2. calculating the expected moles of Hydrazine in the product
3. converting the moles of Hydrazine to grams (expected mass of hydrazine)
4. calculating the percent yield = (25.2 g/expected mass of hydrazine)*100%

Hope it helps!

### Re: Percent yield

Posted: Thu Oct 05, 2017 7:25 pm
question: how do I calculate percent yield?

### Re: Percent yield

Posted: Thu Oct 05, 2017 7:58 pm
percent yield= actual yield (which will be given to you)/theoretical yield

### Re: Percent yield  [ENDORSED]

Posted: Fri Oct 06, 2017 2:23 pm
Hi Jelci!

To calculate percent yield, all you have to do is divide the actual yield by theoretical yield. This will give you a decimal value, which you can then multiply by 100 to get the percent value. To think about this in an easier way just consider how much of your theoretical yield you have produced!

Hope this helps,
Maya

### Re: Percent yield

Posted: Sat Oct 07, 2017 7:01 pm
If it so happens that the theoretical yield and the actual yield have a difference of about 0.99 are we allowed to assume that the actual yield and theoretical yield is the same ?

### Re: Percent yield

Posted: Sun Oct 08, 2017 11:45 am
In most cases even though the difference is small there is still a difference, so you shouldn't assume that the theoretical and actual yield are the same unless it's stated otherwise. If anything this proves that your experiment was highly precise.