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Evgen [1.6K]
2 years ago
5

Question 7

Chemistry
1 answer:
Law Incorporation [45]2 years ago
3 0

Answer:

84.3 g of nitrogen triiodide is the theoretical yield.

Explanation:

Hello there!

In this case, according to the chemical reaction:

N_2 + 3I_2 \rightarrow 2NI_3

It is possible to compute the theoretical yield of nitrogen triiodide by each reactant via stoichiometry as shown below:

m_{NI_3}^{by\ N_2}=4.49gN_2*\frac{1molN_2}{28.01gN_2} *\frac{2molNI_3}{1molN_2}*\frac{394.72gNI_3}{1molNI_3}  =126.55gNI_3\\\\m_{NI_3}^{by\ I_2}=81.3gI_2*\frac{1molI_2}{253.81gI_2} *\frac{2molNI_3}{3molI_2}*\frac{394.72gNI_3}{1molNI_3}  =84.29gNI_3

Therefore, we infer that the smallest amount is the correct theoretical yield as it comes from the limiting reactant, in this case, diatomic iodine as it yields 84.3 g (three significant figures) of nitrogen triiodide as the theoretical yield; incidentally, nitrogen acts as the excess reactant.

Best regards!

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Explanation:

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The question is incomplete, here is the complete question:

At 25°C Henry's Law constant for carbon dioxide gas in water is 0.031 M/atm . Calculate the mass in grams of gas that can be dissolved in 425. mL of water at 25°C and at a partial pressure of 2.92 atm. Round your answer to 2 significant digits.

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<u>Explanation:</u>

To calculate the molar solubility, we use the equation given by Henry's law, which is:

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To calculate the mass of solute, we use the equation used to calculate the molarity of solution:

\text{Molarity of the solution}=\frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}

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