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Basile [38]
3 years ago
11

The sum of three consecutive odd integers is 297. Compute the PRODUCT of the same three consecutive odd integers.

Mathematics
1 answer:
svetoff [14.1K]3 years ago
4 0

Answer:

Step-by-step explanation:

let the odd numbers be x,x+2,x+4

x+x+2+x+4=297

3x+6=297

3x=297-6=291

x=291/3=97

consecutive odd integers are 97,99,101

97×99×101=97×(100-1)×(100+1)=97×(100²-1)=97×100²-97=970000-97=969903

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12 is 80% of what number
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X - the number

80\%x=12 \\
\frac{80}{100}x=12 \\
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x=12 \times \frac{5}{4} \\
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x=15

12 is 80% of 15.
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3 years ago
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The histogram shows the ages of people in a community chorus. How many people in the chorus are 50 or older? Enter your answer i
Vilka [71]

Answer:

13

Step-by-step explanation:

The computation of the number of people in the chorus are 50 or older is as follows

According to the attached figure

In the age of 50 - 60 , there is 8 people

In the age of 60 - 70 , there is 4 people

In the age of 70 -80, there is 1 people

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The same is relevant

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3 years ago
Write the equation of a line in slope intercept form given;<br> (6,-3), (0, 5)
olganol [36]

Answer:

y=(-4/3)x+5

Step-by-step explanation:

so you want to start by using y=mx+b

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m= \frac{5+3}{0-6}

m= \frac{8}{-6}

m= - \frac{4}{3\\}

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3 0
3 years ago
When electricity (the flow of electrons) is passed through a solution, it causes an oxidation-reduction (redox) reaction to occu
oee [108]

Answer:

a. 135 g

b. 60.6 min

Step-by-step explanation:

a. What mass of Cu(s) is electroplated by running 28.5 A of current through a Cu2+ (aq) solution for 4.00 h? Express your answer to three significant figures and include the appropriate units.

The chemical equation for the reaction is given below

Cu²⁺(aq) + 2e⁻ → Cu(s)

We find the number of moles of Cu that are deposited from

nF = It where n = number of moles of electrons, F = Faraday's constant = 96485 C/mol, I = current = 28.5 A and t = time = 4.00 h = 4.00 × 60 min/h × 60 s/min = ‭14,400‬ s

So, n = It/F = 28.5 A × ‭14,400‬ s/96485 C/mol = ‭410,400‬ C/96485 C/mol = 4.254 mol

Since 2 moles of electrons deposits 1 mol of Cu, then 4.254 mol of electrons deposits 4.254 mol × 1 mol of Cu/2 mol = 2.127 mol of Cu

Now, number of moles of Cu = n' = m/M where m = mass of copper and M = molar mass of Cu = 63.546 g/mol

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= 2.127 mol × 63.546 g/mol

= 135.15 g

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b. How many minutes will it take to electroplate 37.1 g of gold by running 5.00 A of current through a solution of Au+(aq)?

The chemical equation for the reaction is given below

Au⁺(aq) + e⁻ → Au(s)

We need to find the number of moles of Au in 37.1 g

So, number of moles of Au = n = m/M where m = mass of gold = 37.1 g and M = molar mass of Au = 196.97 g/mol

So, n = m/M = 37.1 g/196.97 g/mol = 0.188 mol

Since 1 mol of Au is deposited  by 1 moles of electrons, then 0.188 mol of Au deposits 0.188 mol of Au × 1 mol of electrons/1 mol of Au = 0.188 mol of electrons

We find the time it takes to deposit 0.188 mol of electrons that are deposited from

nF = It where n = number of moles of electrons, F = Faraday's constant = 96485 C/mol, I = current = 5.00 A and t = time

So, t = nF/It

= 0.188 mol × 96485 C/mol ÷ 5.00 A

= ‭18173.30‬ C/5.00 A

= 3634.66 s

= 3634.66 s × 1min/60 s

= 60.58 min

≅ 60.6 min to 3 significant figures

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