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2 years ago

How many grams of water contain 2.50 x 10^24 atoms of hydrogen?

Chemistry

1 answer:

Mama L [17]2 years ago

4 0

The mass of water that contains 2.5×10²⁴ atoms of Hydrogen is 74.79 g

<h3>Avogadro's hypothesis </h3>

From Avogadro's hypothesis,

6.02×10²³ atoms = 2 g of H

Therefore,

2.5×10²⁴ atoms = (2.5×10²⁴ × 2) / 6.02×10²³

2.5×10²⁴ atoms = 8.31 g of H

<h3>How to determine the mass of water </h3>

1 mole of water H₂O = (2×1) + 16 = 18 g
Mass of H in 1 mole of water = 2 g

2 g of H is present in 18 g of water.

Therefore,

8.31 g of H will be present in = (8.31 × 18) / 2 = 74.79 g of water.

Thus, 2.5×10²⁴ atoms of Hydrogen is present in 74.79 g of water.

Learn more about Avogadro's number:

brainly.com/question/26141731

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A positively charged subatomic particle

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How many neutrons are in a nucleus of uranium-238?

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146

Explanation:

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3 years ago

A chromium oxide compound contains 104.0 grams of chromium and 48.0 grams of oxygen. What is the most likely empirical formula o

TEA [102]

Answer: Empirical formula of this compound is $Cr_2O_3$

Explanation:

Mass of Cr= 104.0 g

Mass of O = 48.0 g

Step 1 : convert given masses into moles.

Moles of Cr = $\frac{\text{ given mass of Cr}}{\text{ molar mass of Cr}}= \frac{104.0g}{52g/mole}=2moles$

Moles of O = $\frac{\text{ given mass of O}}{\text{ molar mass of O}}= \frac{48.0g}{16g/mole}=3moles$

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For Cr = $\frac{2}{2}=1$

For O = $\frac{3}{2}=1.5$

Converting into simple whole number ratios by multiplying by 2

The ratio of Cr : O= 2: 3

Hence the empirical formula is $Cr_2O_3$

The most likely empirical formula of this compound is $Cr_2O_3$

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3 years ago

If the ph of a 1m naoh solution is 11.3 what is the h+ concentration for that solution?

kotykmax [81]

[H+] = ?

pH = -log[H+]
[H+] = 10^-pH

[H+] = 10^-11,3
[H+] = 5,01 × 10^-12 mol/l

Answer: H+ concentration in this solution equal 5,01 × 10^-12 mol/l.

:-) ;-)

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3 years ago