Answer:
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Answer:
(i) Calculate the average rate of consumption of A in the first 15 seconds of reaction: -8.67X10^(-3) M/s
(ii) Calculate the average rate of production of C in the first 15 seconds of reaction: 0.0.17 M/s
(iii) Calculate the average rate of consumption of A in the last 15 seconds of the reaction: -3x10^(-3) M/s
(iv) Explain the difference between the rates of consumption calculated in (i) and that in (iii): At the beginning the reaction, is fast, then, when time passes, the reaction slows because there are less concentration of the reactants to produce C, so the rate is less.
Explanation:
The general formula to calculate any reaction rate is:
With this formula we can make the calculations, and we can know if r is positive or negative by knowing if we are calculating for a reactant or a product, positive for products, negative for reactants.
(i)
(ii)
In this case we need to multiply delta by 2, because 1 mole of A produces 2 moles of C:
As we know it is a product, r needs to be positive, so we change the sign of the result and we have: 0.017 M/s
(iii)
(iv)
Is already answered in the upper part.
Answer: 1.5% w/v
Solution: (60mL)(2%) = (80mL)(x)
X = 1.5%
Answer:
2 molecular ions are produced and they are charged negatively
Explanation:
If an ion loses an electron then its charge is +1, if it gains an electron then its charge is -1
3 molecular ions lost 2 electrons each, each ion is charged +2
Total charge = 3(+2) = +6
2 molecular ions gained 3 electrons each, each ion is charged -3
Total charge = 2(-3) = -6
1 molarcular ion gained 2 electrons, ion is charged -2
Net charge of the reactants is:
+6 -6 -2 = -2
The net charge of the reactants must be the same as the net charge of the products.
In the products you have 2 neutral molecules (with charge 0) and molecular ions with a charge of magnitude e.
Since the net charge in the reactants is negative, the net charge in the products is also negative
If the number of molecular ions in the products is x then its total charge is:
x*(-1) = -2
x = 2