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3 years ago

A gas occupies a volume of 8.60 L at 45C and 764 torr. What pressure would it occupy if the volume is adjusted to 13.3 L at 20C?

Chemistry

1 answer:

Marizza181 [45]3 years ago

8 0

Answer:

455 Torr

Explanation:

To get the correct answer, we employ the use of the General gas equation.

In its general form, the General gas equation can be written as:

P1V1/T1 = P2V2/T2

Defining the parameters;

P1 = 764 torr

V1 = 8.6L

T1 = 45 degrees Celsius = 273.15+ 45 = 318.15K

P2 = ?

V2 = 13.3L

T2 = 20 degrees Celsius = 273.15 + 20 = 293.15K

Rearranging the equation yields: P2 = P1V1T2/T1V2

Substituting the values:

P2 = (764 * 8.6 * 293.15)/(318.15 * 13.3)

P2= 455.2 Torr

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A 7.83 g sample of hcn contains 0.290 g of h and 4.06 g of n. find the mass of carbon in a sample of hcn with a mass of 3.37 g.

xeze [42]

To obey the Law of Conservation of Mass, the sum of all individual elements of a compound is equal to the mass of the compound. So, if HCN has a mass of 7.83 grams, then

7.83 g = mass of H + mass of C + mass of N

We know the masses of H and N to be 0.290 g and 4.06 g, respectively. Hence, we can find for the mass of C:

7.83 = 0.29 + mass of C + 4.06
mass of C = 3.48 g

As an extension to the Law of Conservation of Mass, there is also a Law of Definite Proportions. According to Dalton's atomic theory, a compound is formed from a fixed ratio of its individual elements. From our previous calculations, we know that the mass ratio of H to C to N is 0.29 g: 3.48 g:4.06 grams. The ratio could also be expressed in percentages. Let's find the mass percentage of Carbon in HCN to be used later:

mass % of Carbon = (3.48 g/7.83 g)*100
mass % of Carbon = 44.44%

So, if you collect a different mass of HCN, say 3.37 g, the corresponding mass of Carbon is equal to:

Mass of Carbon = (3.37)(44.44%)
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