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Kryger [21]
3 years ago
12

A sample of Freon-12 (CF2Cl2) occupies 2.842 x 101 L at 331 K and 2.525 x 102 kPa. Find its volume (in L) at standard temperatur

e and pressure (STP).
Chemistry
1 answer:
Angelina_Jolie [31]3 years ago
3 0
We have to first find the number of moles of Freon-12 in the sample using the ideal gas law equation
PV = nRT
n = \frac{PV}{RT}
since the number of moles at both conditions given and at stp we can write the following formula 
\frac{P1V1}{RT1} =  \frac{P2V2}{RT2}
where parameters for the given conditions are on the left side and parameters for STP conditions are on the right side of the equation
where P1 - pressure - 252.5 kPa
V1 - volume - 28.42 x 10⁻³ m³ 
R - universal gas constant 
T1 - 331 K

STP conditions 
P2 - 101 325 Pa
T2 - 273 K

substituting these values in the equation 

\frac{252 500Pa*28.42*10 ^{-3}m^{3}  }{R*331K} =  \frac{101325 Pa*V}{R*273 K}

V = 58.41 L
Volume at STP is 58.41 L
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One of the reactions in a blast furnace used to reduce iron is shown above. How many grams of Fe2O3 are required to produce 15.5
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Answer : The correct option is, (b) 22.1 g

Solution : Given,

Mass of iron = 15.5 g

Molar mass of iron = 56 g/mole

Molar mass of Fe_2O_3 = 160 g/mole

First we have to calculate the moles of iron.

\text{Moles of Fe}=\frac{\text{Mass of Fe}}{\text{Molar mass of Fe}}=\frac{15.5g}{56g/mole}=0.276moles

Now we have to calculate the moles of Fe_2O_3.

The balanced reaction is,

Fe_2O_3+3CO\rightarrow 2Fe+3CO_2

From the balanced reaction, we conclude that

As, 2 moles of iron obtained from 1 mole of Fe_2O_3

So, 0.276 moles of iron obtained from \frac{0.276}{2}=0.138 mole of Fe_2O_3

Now we have to calculate the mass of Fe_2O_3

\text{Mass of }Fe_2O_3=\text{Moles of }Fe_2O_3\times \text{Molar mass of }Fe_2O_3

\text{Mass of }Fe_2O_3=(0.138mole)\times (160g/mole)=22.08g=22.1g

Therefore, the amount of Fe_2O_3 required are, 22.1 grams.

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