Question

) If you started with 2.3182 g of 3-nitrophthalic acid and had a 93% yield of 3-nitrophthalhydrazide, how many grams of 3-nitrophthalhydrazide were recovered

Answer 1

To calculate the grams of 3-nitrophthalhydrazide recovered from a 93% yield, multiply the theoretical yield of 2.3182 grams by 0.93 to obtain approximately 2.1559 grams of the product.

Step-by-step explanation:

If you started with 2.3182 grams of 3-nitrophthalic acid and had a 93% yield of 3-nitrophthalhydrazide, the actual yield of 3-nitrophthalhydrazide can be calculated by considering the theoretical yield. Theoretical yield is based on a 100% conversion rate from reactants to products. To find the actual yield, you would take the theoretical yield and multiply it by the percent yield.

The calculation would be as follows:

1. 
   
2. Calculate the theoretical yield (assuming that it is the same mass as the reactant, which is typically how these problems are constructed, unless given the stoichiometry of the reaction).
3. 
   
4. Apply the percent yield by multiplying the theoretical yield by 0.93 (which is 93% expressed as a decimal).
5. 
   
6. The result will give you the mass of 3-nitrophthalhydrazide recovered.

For example, if the theoretical yield were 2.3182 g (assuming 1:1 conversion and no other products), then:

Actual yield = Theoretical yield × Percent yield

= 2.3182 g × 0.93

= 2.1559 g

So, you would have recovered approximately 2.1559 grams of 3-nitrophthalhydrazide based on a 93% yield.

Answer 2

Answer: 1.8124 g of 3-nitrophthalhydrazide were recovered.

Step-by-step explanation:

The balanced chemical reaction will be :

`C_8H_5NO_6+N_2H_4\rightarrow C_8H_5N_3O_4+2H_2O`

moles of 3-nitrophthalic acid =
`\frac{\text {given mass}}{\text {molar mass}}=(2.3182g)/(211.13g/mol)=0.0110mol`

As 1 mole of 3-nitrophthalic acid gives = 1 mole of 3-nitrophthalhydrazide

0.0110 moles of 3-nitrophthalic acid gives =
`(1)/(1)* 0.0110=0.0110` mole of 3-nitrophthalhydrazide

mass of 3-nitrophthalhydrazide =
`moles* {\text {molar mass}}=0.0110mol* 177.16g/mol=1.9488g`

As the percentage yield is 93% , the mass of 3-nitrophthalhydrazide recovered =
`(1.9488* 93)/(100)=1.8124g`

Therefore 1.8124 g of 3-nitrophthalhydrazide were recovered.