Which of the following gases will have the highest velocity at a given temperature?
2 answers:
Answer:
C. He
Explanation:
The velocity of a gas can be calculated by the equation:
Where <em>R</em> is the gas constant, <em>T</em> is the temperature, and <em>M</em> the molar mass of the gas.
At a given temperature, the velocity is inversely proportional to the square of the molar mass, so as low is the molar mass, as higher is the velocity. The molar masses are:
Ne = 10 g/mol
O₂ = 2*16 = 32 g/mol
He = 4 g/mol
Cl₂ = 2*35.5 = 71 g/mol
Then, <em>He</em> has the lower molar mass and the highest velocity.
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Answer:
1. 0.97 V
2.
Explanation:
In this case, we can start with the <u>half-reactions</u>:
With this in mind we can <u>add the electrons</u>:
<u>Reduction</u>
<u>Oxidation</u>
The reduction potential values for each half-reaction are:
- 0.69 V
-1.66 V
In the aluminum half-reaction, we have an oxidation reaction, therefore we have to <u>flip</u> the reduction potential value:
+1.66 V
Finally, to calculate the overall potential we have to <u>add</u> the two values:
1.66 V - 0.69 V = <u>0.97 V</u>
For the second question, we have to keep in mind that in the cell notation we put the anode (the oxidation half-reaction) in the left and the cathode (the reduction half-reaction) in the right. Additionally, we have to use "//" for the salt bridge, therefore:
I hope it helps!