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2 years ago

6

How many moles are in 7.46 x 1025 particles of iron

1 answer:

sladkih [1.3K]2 years ago

4 0

Answer:

1 mole of iron =6.023×10^23 particles

1 particles of iron=1/6.023×10^23 mole

7.46×10^25 particles =1/6.023×10^23×7.46×10^25

=1.238×10^48 mole is a required answer.

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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:

$C_{CO_2}=K_H\times p_{CO_2}$

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$K_H$ = Henry's constant = $0.031M/atm$

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$p_{CO_2}$ = partial pressure of carbon dioxide gas = 2.92 atm

Putting values in above equation, we get:

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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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Putting values in above equation, we get:

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