A 150g copper bowl contains 220g of water, both at 20.0oC, A very hot 300 g copper cylinder is dropped into the water, causing t
1 answer:
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Answer:
Approximately .
Explanation:
Cathode is where reduction takes place and anode is where oxidation takes place. The potential of a electrochemical reaction () is equal to
.
There are two half-reactions in this question. and
. Either could be the cathode (while the other acts as the anode.) However, for the reaction to be spontaneous, the value of
should be positive.
In this case, is positive only if
is the reaction takes place at the cathode. The net reaction would be
.
Its cell potential would be equal to .
The maximum amount of electrical energy possible (under standard conditions) is equal to the free energy of this reaction:
,
where
is the number moles of electrons transferred for each mole of the reaction. In this case the value of
as in the half-reactions.
is Faraday's Constant (approximately
.)
.
Answer:
ΔTmin = 3.72 °C
Explanation:
With a 16-bit ADC, you get a resolution of steps. This means that the ADC will divide the maximum 10V input into 65536 steps:
ΔVmin = 10V / 65536 = 152.59μV
Using the thermocouple sensitiviy we can calculate the smallest temperature change that 152.59μV represents on the ADC: