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mr Goodwill [35]
2 years ago
8

The number of integers that satisfy 3|n| +2 <=17 is​

Mathematics
2 answers:
butalik [34]2 years ago
5 0

Answer:

The number of Integers satisfying 3|n| +2 <= 17 is 11.

Step-by-step explanation:

The solution set is: {-5,-4,-3,-2,-1,0,1,2,3,4,5}, which contains 11 elements.

melomori [17]2 years ago
5 0

Answer:

11

Step-by-step explanation:

3|n| + 2 <= 17 subtract 2 by both sides

3|n| <= 15 divide both sides by 3

|n| <= 5

Because it is absolute value negative and positive numbers and 0 fulfill this

So the answer would be 11 because -5, -4, -3, -2, -1, 0, 1, 2, 3, 4, 5.

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G(x)=2x32+c

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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

So, m = n'M

= 2.127 mol × 63.546 g/mol

= 135.15 g

≅ 135 g to 3 significant figures

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

6 0
3 years ago
Graph the function f(x) = 2√x +3.
Nikolay [14]

The graph is shown in the attached image.

8 0
2 years ago
Help me graph this plssss!!! I’d really appreciate it!
Natali [406]

Answer:

Okay so, first put a dot on the number three. Next, go down one and over two from that spot (2, 2) and so on.

Step-by-step explanation:

8 0
2 years ago
Read 2 more answers
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