A 5.2 dm³ gas cylinder containing 822 g of neon is heated until the pressure reaches 232 atm. What is the temperature in °C of the gas?

Question

Quizplus · Accepted Answer

The ideal gas law can be used to solve this problem:PV = nRTwhere P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.We can rearrange this equation to solve for T:T = PV/nRWe are given the following information:P = 232 atmV = 5.2 dm^3n = 822 g / 20.18 g/mol = 40.77 molR = 0.0821 L*atm/(mol*K)Plugging these values into the equation, we get:T = (232 atm * 5.2 dm^3) / (40.77 mol * 0.0821 L*atm/(mol*K))T = 360.95 KConverting to degrees Celsius:T = 360.95 K - 273.15 = 87.80 °CTherefore, the temperature of the gas is 87.80 °C.

A 52 Dm3 Gas Cylinder Containing 822 G of Neon Is

A 52 Dm³ Gas Cylinder Containing 822 G of Neon Is