Answer:
Percent error = 1.3%
Explanation:
Given data:
Actual value of boiling point = 100.0 °C
Measured value = 101.3 °C
Percent error = ?
Solution:
Formula:
Percent error = ( Measured value - Actual value / Actual value ) × 100
Now we will put the values in formula.
Percent error = 101.3 °C - 100.0 °C / 100.0 °C × 100
Percent error = 1.3 °C / 100.0 °C × 100
Percent error = 0.013 × 100
Percent error = 1.3%
Thus, percent error is 1.3.
Break down in to tiny prices as the water hit the tree
Answer:
0.758 V.
Explanation:
Hello!
In this case, case when we include the effect of concentration on an electrochemical cell, we need to consider the Nerst equation at 25 °C:
Whereas n stands for the number of moles of transferred electrons and Q the reaction quotient relating the concentration of the oxidized species over the concentration of the reduced species. In such a way, we can write the undergoing half-reactions in the cell, considering the iron's one is reversed because it has the most positive standard potential so it tends to reduction:
It means that the concentration of the oxidized species is 0.002 M (that of nickel), that of the reduced species is 0.40 M and there are two moles of transferred electrons; therefore, the generated potential turns out:
Beat regards!
The question is missing the table. Here is the complete question.
The tableshows the concentration of a reactant in the mixture over a period of time.
Reactant Concentration
Time (s) Concentration (M)
0 1.8
210 1.2
450 0.8
580 0.6
720 0.4
What is the average rate of reaction over the first 450 seconds?
A. 1.6x M
B. 1.9x M
C. 2.0x M
D. 2.2x M
Answer: D. 2.2x M
Explanation: The average rate of a reaction is the rate of change of the concentrations (of reactants or products) in a period of time:
average = - ΔC/Δt
In this case, concentration is negative because it's related to reactant, since its concentration dimishes while the concentration of product increases.
For the first 450 seconds:
Average =
Average =
Average = 0.0022
or
Average = 2.2x
So, <u>the Average Rate of the reaction is 2.2x</u><u>M</u>