Hello!
<span>We have the following statement data:
</span>
Data:




<span>As the percentage is the mole fraction multiplied by 100:
</span>

<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>



<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

:




<span>
Answer:
</span><span>
b. 320.0 mm hg </span>
Answer:
17
Explanation:
the atomic mass is away protons + neutrons, electrons are neglatable.
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Answer:
0.2 grams
Explanation:
The expression is already in decimal form! Hope this helps.
-Lei
First, we need to calculate the principal quantum number n for this electron, using the equation:
E = (-13.60 eV) / (n x n)
where E is the energy that is used to bound the electron (here, E = - 0.544 eV).
- 0.544 eV = (-13.60 eV) / (n x n)
n x n = (- 13.60 eV) / (- 0.544 eV)
n x n = 25
n = 5
The orbital radius that is equal to the radius of a hydrogen atom is calculated using the equation:
r = 0.053 nm x n x n
r = 0.053 nm x 5 x 5
r = 0.053 nm x 25
r = 1.325 nm