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s2008m [1.1K]
3 years ago
12

Mean Versus Median

Mathematics
1 answer:
Lina20 [59]3 years ago
4 0

Answer:

Kindly check explanation

Step-by-step explanation:

Given the data:

$1.09 $1.29 $1.29 $1.35 $1.39 $1.49 $1.59 $1.79

Average value :

Sarah = $1.37

Andrew = $1.41

Obtaining the median:

(n + 1) / 2

n = number of observations = 8

(8 + 1) / 2 = 9 /2 = 4.5th observation

(4th +. 5th observations) / 2

(1.35 + 1.39) / 2 = $1.37

Finding the mean:

($1.09 + $1.29 + $1.29 + $1.35 + $1.39 + $1.49 + $1.59 + $1.79) /8

$11.28 / 8

= $1.41

Hence, the actual. Average value is the mean value of the data.

The median only gives the value at the middle of the distribution and not the average.

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Evaluate r +<br> Evaluate go when r = 14 and s = 8<br> when r = 14 and s = 8.
serious [3.7K]

Answer:

22

Step-by-step explanation:

thats the answer alright

5 0
3 years ago
Tell weather each equation has one, zero, or infinitely many solutions. -(2x + 2) - 1 = -x - (x + 3)
Anestetic [448]
-(2x+2)-1=-x-(x+3) \\&#10;-2x-2-1=-x-x-3 \\&#10;-2x-3=-2x-3 \\&#10;0=0 \\&#10;always \ true \\ \\&#10;\boxed{\hbox{infinitely many solutions}}
7 0
3 years ago
Given the following rate law, how does the rate of reaction change if the concentration of x is doubled? rate = k [x]2[y]3
tiny-mole [99]

The rate of reaction will increase by a factor of 4. The correct option is D.

<h3>What is the rate of reaction?</h3>

In a reaction mechanism, a chemical reaction is depicted step-by-step. It is composed of separate chemical processes known as elementary stages. An elementary reaction is one that only requires one step to complete.

In an elementary reaction, the orders relative to each reactant are equal to the stoichiometric coefficient of that reactant. A provided rate law must be consistent with both the experimental rate law and the overall rate law that is being suggested.

The rate of reaction will be calculated as below:-

Rate (R) = k[x][y]²

R' = k[x][2y]²

R'=4k[x][y]²

R'=4R

Hence, the rate of reaction will increase by a factor of 4.

The complete question is given below:-

Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]2

A) The rate of reaction will increase by a factor of 2.

B) The rate of reaction will increase by a factor of 5.

C) The rate of reaction will increase by a factor of 4.

D) The rate of reaction will decrease by a factor of 2.

E) The rate of reaction will remain unchanged.

Learn more about the rate of reaction here:

brainly.com/question/8592296

#SPJ4

8 0
2 years ago
Use long division to find each quotient. Show your work
HACTEHA [7]

Answer:

4.4

the only thing that goes in 22 and 5 is 4 and 2 is going to remain because 5 times 4 is 20 so after that add a decimal after the 4 and add a zero next to 22 and bring it down to the 2 so noe the 2 turns into 20 sense 20 goes in 5 4 times the answers is 4.4.

7 0
3 years ago
Perform the indicated operation. (y^4 - 1) ÷ (y + 1)
IceJOKER [234]

Answer:

C

Step-by-step explanation:


6 0
3 years ago
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