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uranmaximum [27]
2 years ago
9

1. How many mg of lithium phosphide are in 18.0 mL of a 1.25 M solution?

Chemistry
1 answer:
Temka [501]2 years ago
6 0

Answer:

1160mg

Explanation:

Molarity = number of moles ÷ volume

According to the information in the question, molarity = 1.25 M, volume = 18.0 mL = 18/1000 = 0.018L

M = n/V

n = M × V

n = 1.25 × 0.018

n = 0.0225moles.

Using mole = mass/molar mass, to find the mass of lithium phosphide (Li3P)

Molar mass of Li3P = 6.9(3) + 31 = 51.7g/mol

mole = mass/molar mass

0.0225 = mass/51.7

mass = 1.16grams.

In milligrams (mg), mass of Li3P = 1.16 × 1000 = 1160mg

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Which statement is incorrect regarding the reaction of benzene with an electrophile? View Available Hint(s) A) The carbocation i
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Answer:

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Explanation:

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The general mechanism is shown in the figure.

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ii) The carbocation intermediate loses a proton from the carbon bonded to the electrophile.

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Thus the wrong statement is

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3 years ago
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Answer:

I can't draw diagrams on this web site but I can do with numbers I think. So an electron is moved from n = 1 to n = 5. I'm assuming I've interpreted the problem correctly; if not you will need to make a correction. I'm assuming that you know the electron in the n = 1 state is the ground state so the 4th exited state moves it to the n = 5 level.

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n = 3 2nd excited state

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Here are the possible spectral lines.

n = 5 to 4, n = 5 to 3, n = 5 to 2, n = 5 to 1 or 4 lines.

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n = 2 to 1 = 1 line. Add 'em up. I get 10.

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To find the E for any transition (delta E) take E for upper n and subtract from the E for the lower n and that gives you delta E for the transition.

So for n = 5 to n = 1, use -Efor 5 -(-Efor 1) = + something which I'll leave for you. You could convert that to wavelength in meters with delta E = hc/wavelength. You might want to try it for the Balmer series (n ending in n = 2). I think the red line is about 650 nm.

Explanation:

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Answer:

a party mix:-) it would be a jar of cashews, peanuts, almonds, ettc.

Explanation:

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