Chemistry, asked by neutron546, 1 year ago

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 Anonymous
11
\text{\underline{\underline{Initial\:conditions:}}}

\sf{V_{1}} = 450 mL

\sf{T_{1}} = 20° C

\sf{T_{1}} = 20 + 273

\sf{T_{1}} = \boxed{293 K}


\text{\underline{\underline{Final\:conditions:}}}

\sf{V_{2}} = ?

\sf{T_{2}} = 50° C

\sf{T_{2}} = 50 + 273

\sf{T_{2}} = \boxed{323 K}


\text{\underline{\underline{According\:to\:Charle's Law}}}:

\boxed{ \frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}} }


Now, substituting the values, in the above formula, we get:

\sf{\frac{V_{1}}{T_{1}} = \frac{V_{2}}{T_{2}}}

\sf{ \frac{450}{293} = \frac{V_{2}}{323}}

\sf{V_{2} = \frac{323 \times 450}{293}}

\sf{V_{2} = \frac{145350}{293}}

\sf{V_{2} = \boxed{496.0 \: mL}}


\text{\underline{\underline{Therefore:}}}

The new volume of the gas at constant pressure is 496.0 mL.


\text{\underline{\underline{Note\:on\:Charle's\:Law}}} :


\bullet 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.


\bullet He observed that for a given mass of a gas, the volume increases with increase in temperature and vice-versa at constant pressure.


\bullet Then he generalised his observations in the form of a law called Charle's Law.


\bullet Charle's Law states that the volume of a given mass of a gas increases or decreases by  \frac{1}{273.15} of the volume at 0°C for each degree rise or fall in temperature respectively, provided pressure is kept constant.

neutron546: superb
Anonymous: Thank you!
Answered by Anonymous
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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