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enyata [817]
2 years ago
15

Determine the scale factor for A ABC to A A'B'C: A. 1/2 B. 10 C. 5 D. 2

Mathematics
2 answers:
Katen [24]2 years ago
7 0

Answer:

2

Step-by-step explanation:

10/5=2

anygoal [31]2 years ago
3 0
D. 2 because scale factor is where you multiply the components of an object, in this case ABC. You are given AC which is 5. The only way 5 could get to 10 is if it is added by 5 or multiplied by 2. We’re using multiplication in this problem so the answer is 2.
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Work out the area of this quarter circle of radius 8 cm.<br> Give your answer in terms of pie
Bess [88]

16pi

Step-by-step explanation:

pi x r² = ans ÷ 4 = Answer for area

Pi×8²=64pi ÷ 4 = 16pi

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

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
Estimate the sum: 1 3/7 + 3 5/9 + 1/2. Show your work.
NISA [10]
Add 1 3/7 and leave it like that, and then do 9x3=27+5=32 so it’s gonna be 32/9 and then calculate the sum into 691/126 or u can divided more into 5 61/126
8 0
2 years ago
Read 2 more answers
Which of these is a complex number?
Ostrovityanka [42]

Answer:

B.

Step-by-step explanation:

That would be B.

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The √(-7/3) is usually written as √(7/3)i where i is √-1, so the complex number is 8/3 + √(7/3)i.

7 0
3 years ago
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The quotient of 1.2 added to a number and 5 is 3.6?
Nat2105 [25]
You would add 5 and 1.2 which gives you 6.2 then you add negative 3.6 which then gives you 3.6.
5 0
3 years ago
Read 2 more answers
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