Answer:
V₂ =541.94 m L.
Explanation:
Given that
V₁ = 500 mL
T₁ = 25°C = 273 + 25 = 298 K
T₂ = 5°C = 273+50 =323 K
The final volume = V₂
We know that ,the ideal gas equation
If the pressure of the gas is constant ,then we can say that
[tex]\dfrac{V_2}{V_1}=\dfrac{T_2}{T_1}[/tex]
[tex]\dfrac{V_2}{V_1}=\dfrac{T_2}{T_1}[/tex]
Now by putting the values in the above equation we get
[tex]V_2=500\times \dfrac{323}{298}\ mL\\V_2=541.94\ mL[/tex]
The final volume of the balloon will be 541.94 m L.
V₂ =541.94 m L.
The final volume of the balloon will be "541.94 mL".
Given:
Volume,
Temperature,
[tex]= 273+25[/tex]
[tex]= 298 \ K[/tex]
[tex]=273+50[/tex]
[tex]=323 \ K[/tex]
By using the Ideal gas equation, we get
→ [tex]\frac{V_2}{V_1} = \frac{T_2}{T_1}[/tex]
or,
→ [tex]V_2 = \frac{T_2\times V_1}{T_1}[/tex]
[tex]= \frac{500\times 323}{298}[/tex]
[tex]= 541.94 \ mL[/tex]
Thus the above approach is correct.
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