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ehidna [41]
2 years ago
12

CFx where x stands for a whole number. Measurements also show that a certain sample of the unknown compound contains 8.5 mol of

fluorine and 2.11 mol of carbon. Write the complete chemical formula for the unknown compound.
Chemistry
1 answer:
4vir4ik [10]2 years ago
6 0

Answer:

CF₄

Explanation:

CFx where x stands for a whole number.

According to the measurements of a certain sample, the molar ratio of fluorine to carbon is 8.5:2.11. We can use this ratio to calculate "x", considering there is 1 mole of carbon in the chemical formula of CFx.

1 mol C × (8.5 mol F/2.11 mol C) = 4 mol F

The chemical formula is CF₄.

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Answer:

Work done in this process = 4053 J

Explanation:

Mass of the gas = 0.092 kg

Pressure is constant = 1 atm = 101325 pa

Initial temperature T_{1} = 200 K

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Gas constant for nitrogen = 297 \frac{J}{kg k}

When pressure of a gas is constant, volume of the gas is directly proportional to its temperature.

⇒ V ∝ T

⇒ \frac{V_{2} }{V_{1} } = \frac{T_{2} }{T_{1} } ------------ ( 1 )

From ideal gas equation P_{1} V_{1} = m R T_{1} ------ (2)

⇒ 101325 × V_{1} = 0.092 × 297 × 200

⇒ V_{1} = 0.054 m^{3}

This is the volume at initial condition.

From equation 1

⇒ \frac{V_{2} }{0.054} = \frac{200}{115}

⇒ V_{2} = 0.094 m^{3}

This is the volume at final condition.

Thus the work done is given by W = P [V_{2} - V_{1} ]

⇒ W = 101325 × [ 0.094 - 0.054]

⇒ W = 4053 J

This is the work done in that process.

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Answer:

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