Answer:
Explanation:
rate of reaction
= -ve change in pressure of ethanol / time
= - (250 -237 )/100 = - 13 / 100 torr/s
= - 0.13 torr/s
next
- (237 - 224 )/100 = - 13 / 100 torr/s
= - .13 torr/s
next
- (224 - 211 )/100 = - 13 / 100 torr/s
= - .13 torr/s
so on
So rate of reaction is constant and it does not depend upon concentration or pressure of reactant .
So order of reaction is zero.
rate of reaction =K [C₂H₅OH]⁰
K is rate constant
K = .13 torr/s
In 900 s decrease in pressure
= 900 x .13 = 117
So after 900s , pressure of ethanol will be
250 - 117 = 133 torr
Answer:
3 m/s
Explanation:
▲
usando la fórmula velocidad = frecuencia multiplicada por la longitud de onda.
v = (1.5)(2)
v= 3 m/s
Answer:
a) galvanic cell
b)electrolytic cell
c) i) K=6.27x10'34
ΔG°=198790 J
ii) K=3.58x10'-34
ΔG°= 191070 J
d) E°=0.278 v
ΔG°= -26827 J
Explanation:
a) There are two kinds of an electrochemical cell, the first is called "galvanic cells", and the second "electrolytic cell".
The fuel cells are capable of produce electric energy through chemical reactions. These reactions are often spontaneous. So, the galvanic cell has a negative value for Gibbs free energy.
b) The electrolytic cell increases the value of Gibbs energy, to positive values, due to the reactions are not spontaneous.
c) i) look image attached
ii) k = look image attached
ΔG° = -nFE° = - 6 X 95500 J/vmole x (-0.33 v)
ΔG° =-191070
d) E°= 0.0592 v/n x lg K
E°= 0.0592V / 1 X log 5.0X10'4
E°= 0.278 v
ΔG° = -nFE° = -1 x 96500 J/ vmole x 0.278v
ΔG° = -26827 J
<h3>Al + O2 -> Al2O3</h3>
Balance it:
<h3>2Al + 3O2 -> 2Al2O3</h3><h3 />
So you need 2 Al and 3 O2 to make 2 Al2O3 (aluminum oxide).
I'm going to assume you have all the O2 you need.
Since 2 mols of Al is needed to make 2 mols of the product, it's a 1:1 ratio. You get as much aluminum oxide for as much aluminum you burn.
So 12.5 mols if there is not a lack of the O2.