A 40.0 mL sample of a gas was found to have a pressure of 1.00 atm at 25 ºC. What will be the new volume?
if the pressure is changed to 0.50 atm at constant temperature?
(b) The temperature of 20. 0 mL of certain gas was changed from 25.0 ºC to 50 ºC at constant pressure. What is the new volume of the gas in mL?
C) The temperature of a certain gas at a pressure of 1 atm was changed from 25.0 ºC to 50 ºC at constant volume. What is the new pressure of the gas in (i) atm (ii) torr?
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This is a case of Isothermal change where you may use the formula --- P₁ V₁ = P₂ V₂ , where Symbols stand for their usual meanings. Suffixes 1 ND 2 CORRESPOND TO INITIAL AND FINAL CONDITION OF THE GAS.
=> 1 * 40 = 0.5 * V₂
=> V₂ = (40/0.5) = 80 ml ................. Answer answer
(b) T₁ = ( 25 + 273 ) = 298 K , T₂ = 50 + 273 = 323 K , V₁ = 20 ml , V₂ = ?
Use formula ----------
......... V₁.............V ₂
=> ----------- = -------------- ........... Iso baric change
.......... T₁ ...........T₂
=> V₂ = V₁ [ T₂ / T₁ ] = 20 [ 323/298 ] = 21.68 ml ............. Answer
(c) Do yourself
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PV = nRT