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kifflom [539]
3 years ago
10

While heating two different samples of water at sea level, one boils at 102°c and one boils at 99.2°c. calculate the percent err

or for each sample from the theoretical 100.0°c?
Chemistry
2 answers:
ivann1987 [24]3 years ago
5 0

<u>Answer:</u> The percentage error of sample 1 of water is 2 % and that of sample 2 is 0.8 %

<u>Explanation:</u>

To calculate the percentage error, we use the equation:

\%\text{ error}=\frac{|\text{Experimental value - Accepted value}|}{\text{Accepted value}}\times 100      ......(1)

  • <u>For sample 1:</u>

Experimental value of temperature = 102°C

Theoretical value of temperature = 100.0°C

Putting values in equation 1, we get:

\%\text{ error}=\frac{|102-100|}{100}\times 100\\\\\%\text{ error}=2\%

  • <u>For sample 2:</u>

Experimental value of temperature = 99.2°C

Theoretical value of temperature = 100.0°C

Putting values in equation 1, we get:

\%\text{ error}=\frac{|99.2-100|}{100}\times 100\\\\\%\text{ error}=0.8\%

Hence, the percentage error of sample 1 of water is 2 % and that of sample 2 is 0.8 %

Evgesh-ka [11]3 years ago
3 0
<span>To find: Sample error in percent
 Solution:
 Formula:
((Experimental value-theoretical value)/theoretical value)*100
 where, theoretical value = 100°c
 and, experimental value = 102°c (sample 1) 99.2°c (sample 2)
 Sample error (in percentage) when boiling level was 102°c = ((102°c-100°c)/100°c)*100 = 2%
 Sample error (in percentage) when boiling level was 99.2°c = ((99.2°c-100°c)/100°c)*100 = -0.8%</span>
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Answer:

D. Ni²⁺  

Explanation:

We know at once that the answer cannot be A or C, because Ni and Cu are already in their lowest oxidation states.

The correct answer must be either B or D.

An electrolytic cell is the opposite of a galvanic cell. In the former, the reaction proceeds spontaneously. In the latter, you must force the reaction to occur.  

One strategy to solve this problem is:

  1. Look up the standard reduction potentials for the half reaction·
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1. Standard reduction potentials

                                E°/V

Cu²⁺ + 2e⁻ ⟶ Cu; 0.3419

Ni²⁺ + 2e⁻ ⟶ Ni;  -0.257

2. Galvanic Cell

We reverse the direction of the more negative half cell and add.

                                       <u>E°/V </u>

Ni ⟶ Ni²⁺ + 2e⁻;           0.257

<u>Cu²⁺ + 2e⁻ ⟶ Cu;      </u>   0.3419

Ni + Cu²⁺ ⟶ Cu + Ni²⁺; 0.599

This is the spontaneous direction.

Cu²⁺ is reduced to Cu.

3. Electrochemical cell

                                        <u>E°/V</u>

Ni²⁺ + 2e⁻ ⟶ Ni;           -0.257

<u>Cu ⟶ Cu²⁺ + 2e⁻;        </u> <u>-0.3419</u>

Cu + Ni²⁺ ⟶ Ni + Cu²⁺; -0.599

This is the non-spontaneous direction.

Ni²⁺ is reduced to Ni in the electrolytic cell.

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Explanation:

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Sonni added 23.79 mL of KOH to 20.00 mL of 0.393 M HF until the equivalence point was reached. What is the concentration of conj
madreJ [45]

Answer:

0.1795 M

Explanation:

From the given information:

The equation is:

\mathbf{HF_{(aq)}+ KOH_{(aq)} \to KF _{(aq)} + H_2O}

From the above equation, the reaction will go to completion due to the strong base:

At the equivalence point, moles of acid (HF) will be equal to moles of base (KOH)

\text{Number of moles = Volume}  \times Molarity

Thus. since moles of HF = moles of KOH

Then; 0.020 × 0.393 M = 0.02379 × (x) M

(x) M = \dfrac{0.02 \times 0.393 \ M}{0.02379}

(x) = 0.3304 M

Thus, the molarity of KOH = 0.3304 M

Using the balanced neutralization reaction;

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Volume = 0.020 L + 0.02379 L

Volume = 0.04379 L

Volume of the solution =  0.04379 L

Therefore; Molarity = \dfrac{moles}{volume}

Molarity = \dfrac{0.00786  \ mol}{0.04379  \ L}

Molarity = 0.17949 mol/L

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