450 ml of oxygen gas at 20°C is heated to 50°C. What is the new volume of the gas at constant pressure?
Answers
Answered by
11
= 450 mL
= 20° C
= 20 + 273
=
= ?
= 50° C
= 50 + 273
=
:
Now, substituting the values, in the above formula, we get:
The new volume of the gas at constant pressure is 496.0 mL.
:
In 1787, French scientist, Jacques Charles studied the effect of change of temperature on the volume of a fixed amount of gas at constant pressure.
He observed that for a given mass of a gas, the volume increases with increase in temperature and vice-versa at constant pressure.
Then he generalised his observations in the form of a law called Charle's Law.
Charle's Law states that the volume of a given mass of a gas increases or decreases by of the volume at 0°C for each degree rise or fall in temperature respectively, provided pressure is kept constant.
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Answered by
1
Answer:
Final volume will be 496 mL.
Explanation:
Given that -
- Initial volume (V1) = 450 mL
- Initial temperature (T1) = 20°C
- Final temperature (T2) = 50°C
To find -
- Final volume (V2)
Solution -
Let's change the temperature into Kelvin.
T1 = 20°C
→ T1 = 20 + 273
→ T1 = 293 K
T2 = 50°€C
→ T2 = 50 + 273
→ T2 = 323 K
Using Charle's law,
→ V1/T1 = V2/T2
→ 450/293 = V2/323
→ V2 = 496 mL
Hence, final volume will be 496 mL.
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