30. GP A 20.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.50 × 10°

Question

30. GP A 20.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.50 × 10° Pa and temperature of 19.0°C (a) Calculate the temperature of the gas in Kelvin. (b) Use the ideal gas law to calculate the number of moles of gas in the tank. (c) Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole. (d) Obtain the num- ber of grams of carbon dioxide in the tank. (e) A fire breaks out, raising the ambient temperature by 224.0 K while 82.0 g of gas leak out of the tank. Calculate the new temperature and the number of moles of gas remaining in the tank.

Explanation / Answer

(a) Temperature in Kelvin = Temperature in deg C + 273.15 = 19 + 273.15 = 292.15 K

(b) Using pV = nRuT

9.5*105 * 20*10-3 = n*8.314*292.15

So, no. of moles, n = 7.82

(c) Atmoic weight of carbon = 12 and oxygen = 16

So, atomic weight of CO2 = 12 + 2*16 = 44 g/mol

(d) Mass m = 44*7.82 = 344.18 g

(e) Gas remaining in the tank = 344 - 82 = 262.18 g

Moles of gas remaining = 262.18/44 = 5.96 moles

New temperature = 224 + 292.15 = 516.15 K

Please rate my answer, good luck...

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