Compute 6.28×1013+7.30×1011.
1 answer:
You might be interested in
Answer:
0.0164 g
Explanation:
Let's consider the reduction of silver (I) to silver that occurs in the cathode during the electroplating.
Ag⁺(aq) + 1 e⁻ → Ag(s)
We can establish the following relations.
- 1 A = 1 C/s
- The charge of 1 mole of electrons is 96,468 C (Faraday's constant)
- 1 mole of Ag(s) is deposited when 1 mole of electrons circulate.
- The molar mass of silver is 107.87 g/mol
The mass of silver deposited when a current of 0.770 A circulates during 19.0 seconds is:
Answer: Rate law=, order with respect to A is 1, order with respect to B is 2 and total order is 3. Rate law constant is
Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
k= rate constant
x = order with respect to A
y = order with respect to A
n = x+y = Total order
a) From trial 1: (1)
From trial 2: (2)
Dividing 2 by 1 :
therefore y=2.
b) From trial 2: (3)
From trial 3: (4)
Dividing 4 by 3:
, x=1
Thus rate law is
Thus order with respect to A is 1 , order with respect to B is 2 and total order is 1+2=3.
c) For calculating k:
Using trial 1:
.