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Zigmanuir [339]
2 years ago
6

A measure of how close a series of measurements are to one another.

Chemistry
1 answer:
ser-zykov [4K]2 years ago
7 0

Answer: Precision is a measure of how close a series of measurements are to one another. Precise measurements are highly reproducible, even if the measurements are not near the correct value. Darts thrown at a dartboard are helpful in illustrating accuracy and precision

Explanation: a if this wrong u fault u gave no detail

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During oxidation of ethanol to ethanol, the ethanol formed was found to be contaminated with unconverted ethanol, describe how y
Dafna1 [17]

<u><em>The process of how we would obtain </em></u><u><em>ethanal</em></u><u><em> </em></u><u><em>free</em></u><u><em> from ethanol is described in the explanations below. </em></u>

<u><em /></u>

  • In Chemistry, Ethanol undergoes oxidation in the presence of sodium dichromate plus sulphuric acid to yield ethanal and water.

The procedure for achieving this in the laboratory is as follows;

  • Step 1; Measure a quantity of a solution of sodium dichromate acidified in a dilute sulphuric acid and pour into a test tube.

  • Step 2; Add excess <em>ethanol</em>. This is because if we don't do so there will be plenty of oxidizing agent to carry out a second operation which changes the aldehyde to ethanoic acid. However, we need only the aldehyde.

  • Step 3; When the aldehyde ethanal begins to form which will be evident by the change in the colour of solution from <em>orange to green</em>, then the mixture should be distilled from the test tube and tbethe aldehyde collevted so that it doesn't undergo additional oxidation into ethanoic acid.

Read more at; https://brainly.in/question/18574624

4 0
2 years ago
Read 2 more answers
How much ice (in grams) would have to melt to lower the temperature of 353 mL of water from 26 ∘C to 6 ∘C? (Assume the density o
Rashid [163]

Answer:

The mass of ice required to melt to lower the temperature of 353 mL of water from 26 ⁰C to 6 ⁰C is 85.4197 kg

Explanation:

Heat gain by ice = Heat lost by water

Thus,  

Heat of fusion + m_{ice}\times C_{ice}\times (T_f-T_i)=-m_{water}\times C_{water}\times (T_f-T_i)

Where, negative sign signifies heat loss

Or,  

Heat of fusion + m_{ice}\times C_{ice}\times (T_f-T_i)=m_{water}\times C_{water}\times (T_i-T_f)

Heat of fusion = 334 J/g

Heat of fusion of ice with mass x = 334x J/g

For ice:

Mass = x g

Initial temperature = 0 °C

Final temperature = 6 °C

Specific heat of ice = 1.996 J/g°C

For water:

Volume = 353 mL

Density (\rho)=\frac{Mass(m)}{Volume(V)}

Density of water = 1.0 g/mL

So, mass of water = 353 g

Initial temperature = 26 °C

Final temperature = 6 °C

Specific heat of water = 4.186 J/g°C

So,  

334x+x\times 1.996\times (6-0)=353\times 4.186\times (26-6)

334x+x\times 11.976=29553.16

345.976x = 29553.16

x = 85.4197 kg

Thus,  

<u>The mass of ice required to melt to lower the temperature of 353 mL of water from 26 ⁰C to 6 ⁰C is 85.4197 kg</u>

7 0
3 years ago
How many formula units are found in 2.10 gram of Mgo? (No units<br> needed.)
disa [49]

Answer:

84.63924

Explanation:

one moles equals 40.30440

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What do Van der Waals forces do?
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Weaken London dispersion forces and stronger dipole dipole forces
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