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Luda [366]
1 year ago
13

Rounding to the nearest

Chemistry
2 answers:
Romashka [77]1 year ago
8 0

For calculating mean value, add up all of the values then divide by the number of them. 815/9 is about 90.6

<h3>What is mean value?</h3>

The mean refers to the average of a set of values. The mean can be computed in a number of ways, including the simple arithmetic mean (add up the numbers and divide the total by the number of observations), the geometric mean, and the harmonic mean.

Moreover, the mean can be used to represent the typical value and therefore serves as a yardstick for all observations. For example, if we would like to know how many hours on average an employee spends at training in a year, we can find the mean training hours of a group of employees.

Hence, the mean can be calculated only for numeric variables, no matter if they are discrete or continuous. It's obtained by simply dividing the sum of all values in a data set by the number of values.

Learn more about mean value:

brainly.com/question/14882017

#SPJ2

Ganezh [65]1 year ago
8 0
Add up all of the values then divide by the number of them. 815/9 is about 90.6
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2' A mixture containing 2.75 gof ammonium chloride (NH4cl) in 5.0 g of water was heated to dissolve the solid and then allowed t
Trava [24]

Answer:

55g NH₄Cl / 100g Water

Explanation:

Solubility of a substance define the amount of solute per solvent in a saturated solution. The solution can dissolve additional solute if heated.

In the problem, as the first crystal appears at 61°C the solubility in this temperature is the concentration of the solution, that is:

2,75g NH₄Cl / 5,0g water ₓ 100 = <em>55g NH₄Cl / 100g Water</em>

<em></em>

I hope it helps!

6 0
3 years ago
according to john dalton’s observations, when elements combine in a compound, a. the ratio of their masses is always the same. b
yawa3891 [41]

<u><em>Answer:</em></u>

  • The correct answer is a.
  • The ratio of their masses is always the same

<u><em>Explanation:</em></u>

  • Dalton law was based on law of conservation of masses and law of conservation definite proportional. So here , it is cleared that the ratio of their masses should be always same.
8 0
3 years ago
Read 2 more answers
I don't understand the question
s344n2d4d5 [400]
How does the picture show that the inner core spins faster than the outer core?
7 0
4 years ago
Read 2 more answers
Why would "not flammable" be a chemical property rather than a physical property ?
Dmitrij [34]
When something is flammable, it burns and burning is a chemical property since the compounds are being broken down and gas is released. If something is non-falammable, it would then be a chemical property as well since the chemical makeup would not be broken by a flame. (I apologize if my answer is a bit broad or unspecific)
4 0
3 years ago
PLEASE HELP! 25 POINTS!!!! I got the #1, just not #2 and #3. An industrial chemical company has opened a new plant that will pro
podryga [215]

Answer :

Part 1 : Balanced reaction, 3H_2(g)+N_2(g)\rightarrow 2NH_3(g)

Part 2 : The theoretical yield of NH_3 gas = 440.96 g

Part 3 : The % yield of ammonia is 90.03 %

Solution : Given,

Mass of N_2 = 475 g

Molar mass of N_2 = 28 g/mole

Molar mass of NH_3 = 17 g/mole

Experimental yield of NH_3 = 397 g

<u>Answer for Part (1) :</u>

The balanced chemical reaction is,

3H_2(g)+N_2(g)\rightarrow 2NH_3(g)

<u>Answer for Part (2) :</u>

First we have to calculate the moles of N_2.

\text{Moles of }N_2=\frac{\text{ Mass of }N_2}{\text{ Molecular mass of }N_2}=\frac{475g}{28g/mole}=16.96moles

From the given reaction, we conclude that

1 moles of N_2 gas react to give 2 moles of NH_3 gas

16.96 moles of N_2 gas react to give \frac{2}{1}\times 16.96=33.92 moles of NH_3 gas

Now we have to calculate the mass of NH_3 gas.

\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3

\text{ Mass of }NH_3=(33.92moles)\times (17g/mole)=440.96g

Therefore, the theoretical yield of NH_3 gas = 440.96 g

<u>Answer for Part (3) :</u>

Formula used for percent yield :

\% \text{ yield of }NH_3=\frac{\text{ Experimental yield of }NH_3}{\text{ Theoretical yield of }NH_3}\times 100

\% \text{ yield of }NH_3=\frac{397g}{440.96g}\times 100=90.03\%

Therefore, the % yield of ammonia is 90.03 %

3 0
3 years ago
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