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VARVARA [1.3K]
3 years ago
5

Sex-linked disorders occur more frequently in males than females because males have two X chromosomes and females have two Y chr

omosomes. is this true or false?
Chemistry
2 answers:
Vilka [71]3 years ago
5 0
This is false because males have 1 X and 1 Y chromosome. It's females who have 2 X chromosomes. So, it's false.
zepelin [54]3 years ago
5 0
This is false because a male has an X and a Y chromosome while the female have 2 x chromosomes.
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Which best describes the effect of j.j. thompsons theory
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What will happen to the chemical equilibrium if NH4Cl is added to this solution?
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The answer to this item depends entirely to the chemical reaction. If the compound, NH4Cl, is in the left hand side of the reaction, when it is added, the reaction will shift to the left. In the same manner, when the compound is in the right-hand side of the reaction, the reaction will shift to the right.

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The atomic mass of potassium is 39.1. What is the mass of 6.02 × 1023 atoms of potassium? . . A.. 39.1 mg. . . . . B.. 39.1 g. .
Sholpan [36]
Atomic mass of Potassium = Mass of 1 atom of Potassium = 39.1 amu
Then
Mass of 6.02 x 1023 atoms of potassium = 39.1 x 6.02 x 1023 amu
                                                                  = 
We already know that
1 mole = 6.02 x 1023 atoms
Also
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Then
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3 years ago
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Melamine, C3N3(NH2)3, is used in adhesives and resins. It is manufactured in a two-step process: CO(NH2)2(l) → HNCO(l) + NH3(g)
svetlana [45]

Answer:

43.13Kg of melamine

Explanation:

The problem gives you the mass of urea and two balanced equations:CO(NH_{2})_{2}_{(l)}=HNCO_{(l)}+NH_{3}_{(g)}

6HNO_{l}=C_{3}N_{3}(NH_{2})_{3}_{(l)}+3CO_{2}_{(g)}

First we need to calculate the number of moles of urea that are used in the reaction, so:

molar mass of urea = 60.06\frac{g}{mol}*\frac{1kg}{1000g}=0.06006\frac{Kg}{mol}

The problem says that you have 161.2Kg of urea, so you take that mass of urea and find the moles of urea:

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Now from the stoichiometry you have:

2684 moles of urea*\frac{1molofHNCO}{1molurea}*\frac{1molofmelamine}{6molesofHNCO} = 447 moles of melamine

The molar mass of the melamine is 126.12\frac{g}{mol} so we have:

447molesofmelamine*\frac{126.12g}{1molofmelamine} = 5637.64 g of melamine

Converting that mass of melamine to Kg:

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Finally we need to calculate the mass of melamine with a yield of 76.5%, so we have:

%yield = 100*(Actual yield of melamine / Theoretical yield of melamine)

Actual yield of melamine = \frac{76.5}{100}*56.38Kg = 43.13Kg of melamine

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3 years ago
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