All categories

2 years ago

The accepted value is 1.43. Which correctly describes this student’s experimental data?

Chemistry

2 answers:

Yuliya22 [10]2 years ago

7 0

Answer: neither accurate nor precise

Explanation:

Accuracy is defined as how close the measured value is to a standard value. For example if the given volume of water is 20 ml and the two measured values are 19 ml and 18 ml then the former measured value is more accurate than the later.

Precision is defined as how measured values are close to each other. For example, if the length of the wire of 10 m. If the first person measures the length of the same wire thrice and got values 9.7, 9.8 and 9.75 m whereas the second person got values 9.5 , 9.6 and 9.8. In such a case the first person’s measured value is more precise.

Thus as the accepted value is 1.43 and measured values are 1.29 , 1.93 and 0.88 , the experimental data is neither accurate nor precise.

Natalija [7]2 years ago

4 0

Answer:

Neither accurate nor precise

Explanation:

The values were not near or even the same as the accepted value thus making it neither accurate nor precise.

You might be interested in

What is the number of electrons in the outermost energy level of an oxygen atom

Romashka [77]

6 Is the answer. hope you pass

5 0

3 years ago

Read 2 more answers

Please help! ill make a free point question and brainliest if you answer this right!

Alexxx [7]

Answer:

thxx

Explanation:

this helps a lot <3

6 0

2 years ago

Read 2 more answers

Consider a voltaic cell where the anode half-reaction is Zn(s) → Zn2+(aq) + 2 e− and the cathode half-reaction is Sn2+(aq) + 2 e

Sonbull [250]

Answer:

Option (B) is correct

Explanation:

Oxidation: $Zn\rightarrow Zn^{2+}+2e^{-}$

Reduction: $Sn^{2+}+2e^{-}\rightarrow Sn$

---------------------------------------------------------------------------

Overall: $Zn+Sn^{2+}\rightarrow Zn^{2+}+Sn$

Nernst equation for this cell reaction at $25^{0}\textrm{C}$ :

$E_{cell}=(E_{Sn^{2+}\mid Sn}^{0}-E_{Zn^{2+}\mid Zn}^{0})-\frac{0.059}{n}log\frac{[Zn^{2+}]}{[Sn^{2+}]}$

Where, n is number of electron exchanged and species inside third bracket represents concentrations in molarity.

Here, n = 2, $E_{cell}=0.660V$ and $[Zn^{2+}]=2.5\times 10^{-3}M$

So, plug in all the given values into above equation:

$0.660V=(-0.136V+0.76V)-\frac{0.059}{2}log\frac{2.5\times 10^{-3}M}{[Sn^{2+}]}$

So, $[Sn^{2+}]=4.2\times 10^{-2}M$

As the value "0.059" varies from literature to literature and $4.2\times 10^{-2}M$ is most closest to $3.3\times 10^{-2}M$ therefore option (B) is correct.

8 0

2 years ago

12 moles of Cu is how many grams of Cu?

exis [7]

Answer:

762.60 g

Explanation:

In order to convert from moles of a substance into grams, we need to multiply the number of moles by the substance's molar mass:

Moles * Molar Mass = Grams

With the above information in mind, we can <em>use the data given by the problem</em> and <u>calculate how many grams are there in 12 moles of Cu</u>:

12 mol * 63.55 g/mol = 762.60 g

3 0

2 years ago

In a bond Between fluorine and bromine which direction will the bond dipole point?

maria [59]

Answer: Bond Polarity | Chemistry for Non-Majors - Lumen Learning

Explanation:

7 0

3 years ago