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nika2105 [10]
3 years ago
11

The forensic technician at a crime scene has just prepared a luminol stock solution by adding 16.0 g of luminol into a total vol

ume of 75.0 mL of H2O. What is the molarity of the stock solution of luminol?
Chemistry
1 answer:
nikitadnepr [17]3 years ago
6 0

 The  molarity  of  the stock solution of  luminol  is 1.2 M


 <u><em>calculation</em></u>

step 1:  find the moles  of  luminol  using   (moles=  mass/molar mass)  formula


molar  mass  of Luminol= 177 g/mol

moles  is therefore= 16.0 g/ 177  g/mol=0.0904 moles


Step  2:  find the molarity  using (molarity= moles/volume in liters)  formula

     convert  Ml  into liters =  75.0/1000= 0.075 L

  molarity is therefore= 0.0904 moles/ 0.075 L= 1.2M

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Explanation:

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In class we derived the Gibbs energy of mixing for a binary mixture of perfect gases. We also discussed that the same result is
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Answer:

Attached below

Explanation:

Free energy of mixing = ΔGmix = Gf - Gi

attached below is the required derivation of the

<u>a) Molar Gibbs energy of mixing</u>

ΔGmix = Gf - Gi

hence : ΔGmix = ∩RT ( X1 In X1 + X2 In X2 + X3 In X3 + ------- )

<u>b) molar excess Gibbs energy of mixing</u>

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4 0
3 years ago
Which is a reason that a chemical engineer would use a rate law for a reaction in a chemical plant?
Harrizon [31]
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3 years ago
Read 2 more answers
Quinine, an antimalarial drug, is 8.63% nitrogen. There are two nitrogen atoms per molecule. What is the molecular weight of qui
Furkat [3]

Answer:

324.18 g/mol

Explanation:

Let the molecular mass of the antimalarial drug, Quinine is x g/mol

According to question,

Nitrogen present in the drug is 8.63% of x

So, mass of nitrogen = \frac {8.63}{100}\times x

Also, according to the question,

2 atoms are present in 1 molecule of the drug.

Mass of nitrogen = 14.01 amu = 14.01 g/mol (grams for 1 mole)

So, mass of nitrogen = 14.01×2 = 28.02

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\frac {8.63}{100}\times x=28.02

solving for x, we get:

<u>x = 324.18 g/mol</u>

6 0
3 years ago
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