What is the partial pressure of ethane, pethane, in the flask?
1 answer:
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Answer:
D. 18,800 J/mol
Explanation:
We need to use the Arrhenius equation to solve for this problem:
, where k is the rate constant, A is the frequency factor,
is the activation energy, R is the gas constant, and T is the temperature in Kelvins.
We want to find the value of , so let's plug some of the information we have into the equation. The gas constant we can use here is 8.31 J/mol-K.
At 0°C, which is 0 + 273 = 273 Kelvins, the rate constant k is . So:
At 20°C, which is 20 + 273 = 293 Kelvins, the rate constant k is . So:
We now have two equations and two variables to solve for. We just want to find Ea, so let's write the first equation for A in terms of Ea:
Plug this in for A in the second equation:
After some troublesome manipulation, the answer should come down to be approximately:
Ea = 18,800 J/mol
The answer is thus D.
Answer: We take 20 ml of 1.0 M fruit drink and add 80 ml of water to get 100 ml of 0.2 M solution.
Explanation:
According to the neutralization law,
where,
= molarity of stock solution = 0.2 M
= volume of stock solution = 100 ml
= molarity of resulting solution = 1.0 M
= volume of resulting solution = ?
Now put all the given values in the above law, we get the volume of resulting solution.
Therefore, the volume of 1.0 M required is 20 ml.
We take 20 ml of 1.0 M fruit drink and add 80 ml of water to get 100 ml of 0.2 M solution.