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Klio2033 [76]
3 years ago
6

How many moles of zinc are in 4.70 kg of zinc?

Chemistry
2 answers:
Semmy [17]3 years ago
7 0

Answer:

There are 71.89 moles of Zinc in 4.70kg of Zinc

Explanation:

Information given;

- Calculate Number of moles

- Mass of Zinc

Before proceeding, it is important to know the definition of what molar mass is. Molar mass is defined as the mass in grams of one mole of a substance.

So it means one mole of Zinc would contain the molar mass in g.

The molar mass of Zinc is given as; 65.38g/mol

How many moles then in 4.70kg?

Upon converting to g, we have 4.7 *1000 = 4700g

1 mol = 65.38g

x mol = 4700g

Cross multiplication yields;

x = (1* 4700) / 65.38

x = 71.89 moles

It means that there are 71.89 moles of Zinc in 4.70kg of Zinc

faust18 [17]3 years ago
6 0
First we convert kg to g
1kg =1000g
4.70=x(gram)
4.70×1000÷1=4700g
now:
number of moles=mass÷molarmass
number of moles=4700÷65.4
number of moles=71.86moles.
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A sample of nitrogen gas is at a temperature of 50 c and a pressure of 2 atm. If the volume of the sample remains constant and t
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The new temperature of the nitrogen gas is 516.8 K or 243.8 C.

Explanation:

Gay-Lussac's law indicates that, as long as the volume of the container containing the gas is constant, as the temperature increases, the gas molecules move faster. Then the number of collisions with the walls increases, that is, the pressure increases. That is, the pressure of the gas is directly proportional to its temperature.

Gay-Lussac's law can be expressed mathematically as follows:

\frac{P}{T} =k

Where P = pressure, T = temperature, K = Constant

You want to study two different states, an initial state and a final state. You have a gas that is at a pressure P1 and at a temperature T1 at the beginning of the experiment. By varying the temperature to a new value T2, then the pressure will change to P2, and the following will be fulfilled:

\frac{P1}{T1} =\frac{P2}{T2}

In this case:

  • P1= 2 atm
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  • P2= 3.2 atm
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Replacing:

\frac{2 atm}{323 K} =\frac{3.2 atm}{T2}

Solving:

T2*\frac{2 atm}{323 K} =3.2 atm

T2=3.2 atm*\frac{323 K}{2 atm}

T2= 516.8 K= 243.8 C

<u><em>The new temperature of the nitrogen gas is 516.8 K or 243.8 C.</em></u>

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