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LenaWriter [7]
3 years ago
6

PLEASE ASNWR ASAP

Chemistry
1 answer:
Vikki [24]3 years ago
4 0
34.95 atm

lol i hope i’m not too late



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) If you started with 2.3182 g of 3-nitrophthalic acid and had a 93% yield of 3-nitrophthalhydrazide, how many grams of 3-nitrop
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Answer: 1.8124 g of 3-nitrophthalhydrazide were recovered.

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}}=\frac{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 = \frac{1}{1}\times 0.0110=0.0110 mole of 3-nitrophthalhydrazide

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

As the percentage yield is 93% , the mass of 3-nitrophthalhydrazide recovered = \frac{1.9488\times 93}{100}=1.8124g

Therefore 1.8124 g of 3-nitrophthalhydrazide were recovered.

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Two reasons that a plant from a rain forest would not survive in a desert home?
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Explanation: I hope this helped you.

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m = mass (kg)

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h = height (meters)

= 90 * 9.8 * 5000

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