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dsp73
3 years ago
13

Determine the number of atoms in 1.70 ml of mercury. (the density of mercury is 13.5 g/ml.)

Chemistry
1 answer:
marishachu [46]3 years ago
8 0

<span>To determine the number of atoms in 1.70ml of mercury, we have to determine the moles of mercury.</span>

<span>First find the mass in grams by using the formula:</span>

<span>Mass = volume x density</span>

<span>(1.70 mL Hg) x (13.5 g/mL) = 22.95 g Hg </span>

<span>Now find number of moles;</span>

<span>
(22.95 g Hg) x (1 mol Hg/200.59 g/mol) = 0.1144 mol Hg </span>

<span>For number of atoms multiply with Avogardro's number that is 6.023 x 10</span>²³

<span>
<span>(0.1144 mol Hg) x (6.023 x 10</span></span>²³ atoms/mol) = 6.89 x 10²² atoms Hg 

So, there is 6.89 x 10²² atoms of mercury are present in 1.70ml of mercury.

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6 0
2 years ago
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A mixture of gases with a pressure of 800.0 mm hg contains 60% nitrogen and 40% oxygen by volume. what is the partial pressure o
klasskru [66]
Hello!

<span>We have the following statement data:
</span>
Data:
P_{Total} = 800 mmHg
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P\% O_{2} = 40\%
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<span>As the percentage is the mole fraction multiplied by 100:

</span>P =  X_{ O_{2} }*100

<span>The mole fraction will be the percentage divided by 100, thus:
</span><span>What is the partial pressure of oxygen in this mixture? 
</span>
X_{ O_{2} }  =  \frac{P}{100}
X_{ O_{2}} =  \frac{40}{100}
\boxed{X_{ O_{2}} = 0.4}


<span>To calculate the partial pressure of the oxygen gas, it is enough to use the formula that involves the pressures (total and partial) and the fraction in quantity of matter:
</span>
In relation to O_{2} :

\frac{P O_{2} }{P_{total}} = X_O_{2}
\frac{P O_{2} }{800} = 0.4
P_O_{2} = 0.4*800
\boxed{\boxed{P_O_{2} = 320\:mmHg}}\end{array}}\qquad\quad\checkmark
<span>
Answer:
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