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2 answers:
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Answer:
1.65 L
Explanation:
The equation for the reaction is given as:
A + B ⇄ C
where;
numbers of moles = 0.386 mol C (g)
Volume = 7.29 L
Molar concentration of C =
= 0.053 M
A + B ⇄ C
Initial 0 0 0.530
Change +x +x - x
Equilibrium x x (0.0530 - x)
where
K is given as ; 78.2 atm-1.
So, we have:
Using quadratic formula;
where; a = 78.2 ; b = 1 ; c= - 0.0530
= or
= or
= 0.0204 or -0.0332
Going by the positive value; we have:
x = 0.0204
[A] = 0.0204
[B] = 0.0204
[C] = 0.0530 - x
= 0.0530 - 0.0204
= 0.0326
Total number of moles at equilibrium = 0.0204 + 0.0204 + 0.0326
= 0.0734
Finally, we can calculate the volume of the cylinder at equilibrium using the ideal gas; PV =nRT
if we make V the subject of the formula; we have:
where;
P (pressure) = 1 atm
n (number of moles) = 0.0734 mole
R (rate constant) = 0.0821 L-atm/mol-K
T = 273.15 K (fixed constant temperature )
V (volume) = ???
V = 1.64604
V ≅ 1.65 L
Answer:
-) Oxidizing agent:
-) Reducing agent:
Explanation:
The first step is separate the reaction into the <u>semireactions</u>:
A.
B.
If we want to balance in <u>basic medium </u>we have to follow the rules:
1. We adjust the oxygen with
2. We adjust the H with
3. We adjust the charge with
Lets balance the first semireaction A. :
Now, lets balance semireaction B:
Finally, we have to add the two semireactions:
_________________________________________
_________________________________________
Cancel out the species on both sides:
Simplifying the equation :
The is <u>oxidized</u> therefefore is the <u>reducing agent</u>. The
is<u> reduced</u> therefore is the <u>oxidizing agent</u>.