According to the stoichiometry the CO2 formed is 1/2 the moles of H2O. So take the moles of CO2 as 5moles.
n=m/M
Where :
n = mole
m = mass
M = molar mass
Molar mass of CO2 = 44gmol^-1
Therefore mass = 5mol× 44gmol^-1= 220g
Subtract the number of electrons from the protons. neutrons have no charge so those don't matter in the formula
The percent error of Chemistry student : 7.4%
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Further explanation
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Given
40 °C measurement
Required
The percent error
Solution
% Error : difference between the theoretical value and the actual value
or
% Error : Absolute Error / Accepted Value
Absolute Error = Measured Value - Accepted Value
% Error for Chemistry student :
1. Subtract the measurement value with the accepted value
= 40 °C - 43.2 °C
= -3.2 °C
2. Divide by the accepted value, and multiply by 100
= |-3.2/43.2| x 100%
= 7.4%
Answer: wait im gonna search some info.
Explanation:I come back with an asnwer for you
At anode,
Cd-----> + 2
At cathode,
+ 2e -----> Ni
Overall reaction,
+ Cd(s) ------> + Ni K=1.17
(aq) (aq) (s)
By nernst equation,
E= - Log K
Where,
F=96500c/mol
M=2
T=298K
E=Zero at equilibrium
R=8.314 J
0= - Log(1.17)
= 0.150v
what is nernst equation?
The Nernst equation is a chemical thermodynamical relationship used in electrochemistry that enables the determination of a reaction's reduction potential (half-cell or full-cell reaction) from the standard electrode potential, absolute temperature, the number of electrons involved in the oxydo-reduction reaction, and activities (often approximated by concentrations) of the chemical species undergoing reduction and oxidation, respectively. It was given the equation's original name in honor of the German physical scientist Walther Nernst.
The link between cell potential, standard potential, and the behaviors of electrically active (electroactive) species is described by the Nernst equation. It links the standard cell potential to the effective concentrations (activities) of the reaction's constituent parts.
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