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Gemiola [76]
3 years ago
11

If you were a biologist counting very large numbers of cells as part of your research, give several reasons why you might prefer

to record your cell counts in scientific notation instead of standard notation.
Mathematics
1 answer:
never [62]3 years ago
4 0

Answer:

I would prefer scientific because depending how big a the number is scientific makes it the number visible smaller

Step-by-step explanation:

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Answer:

33.6 x 3.1 = 104.16

Step-by-step explanation:

To multiply decimals, first multiply as if there is no decimal. Next, count the number of digits after the decimal in each factor. Finally, put the same number of digits behind the decimal in the product.

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2 (3x+1)=17-3 (x-17)
elena-14-01-66 [18.8K]
<h2>Answer:</h2>

x =  \frac{22}{3}

<h3>alternative form:</h3>

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<h2>Step-by-step explanation:</h2>

2(3x + 1) = 17 - 3( x - 17) \\ distribute \\  \\ 6x + 2 = 17 - 3x  + 51 \\ add \: 3x \: from \: both \: sides \\  \\ 9x + 2 = 17  +  51 \\ add \: 17 \: to \: 51 \\  \\ 9x + 2 = 68 \\ subtract \: 2 \: from \: both \: sides \\  \\ 9x = 66 \\  divide \: both \: sides \: by \: 9 \\  \\ x =  \frac{22}{3}

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3 years ago
use a compass to draw a circle and cut it out fold the circle three times as shown to get equal wedges unfold and shade one half
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Step-by-step explanation:

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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
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