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What volume will 500 mL of gas at 20 c and a pressure of 420 mm Hg occupy if the temperature is reduced to 80 c and the pressure increased to 650 mm Hg?
Wiki User
∙ 11y ago
V = k*T/P
Apart from the fact that a change in temperature from 20C to 80C cannot be described as a reduction,
V2 = V1 * T2P1/T1P2
= 500*(273.15+80)*420/[(273.15+20)*650]
= 500*353.15*420/(293.15*650)
= 289.2 mL
Wiki User
∙ 11y ago
To solve, use the combined gas law: (P1V1/T1) = (P2V2/T2). Plug in the initial conditions (P1 = 420 mm Hg, V1 = 500 mL, T1 = 20°C), and the final conditions (P2 = 650 mm Hg, T2 = 80°C) to find V2, the final volume. Remember to convert temperatures to Kelvin by adding 273 to the Celsius temperature.
Wiki User
∙ 12y ago490ml
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