CaSO3 (s) → → → → CaO (s) + SO2 (g)
What mass of CaSO3 must have been present initially to produce 14.5 L of SO2 gas at a temperature of 12.5°C and a pressure of 1.10 atm?

Question

30-04-2016
Chemistry

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CaSO3 (s) → → → → CaO (s) + SO2 (g)
What mass of CaSO3 must have been present initially to produce 14.5 L of SO2 gas at a temperature of 12.5°C and a pressure of 1.10 atm?

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JaySL JaySL · Answer 1 · 2016-04-30T22:59:52+02:00

Using the ideal gas law, the number of moles SO2 is equal to PV/RT, or pressure times volume divided by the gas constant and temperature. This is 14.5*1.1/((2.5+279.15)*.082), or 0.66 moles. Since one mole CaSO3 is consumed for every mole SO2 generated, 0.66 moles of CaSO3 are consumed. CaSO3 has a molar mass of 40+32+16*3=120 grams, so .66 moles of CaSO3 is equal to 80 grams, our final answer.

CaSO3 (s) → → → → CaO (s) + SO2 (g) What mass of CaSO3 must have been present initially to produce 14.5 L of SO2 gas at a temperature of 12.5°C and a pressure of 1.10 atm?

Respuesta :

Otras preguntas

CaSO3 (s) → → → → CaO (s) + SO2 (g)
What mass of CaSO3 must have been present initially to produce 14.5 L of SO2 gas at a temperature of 12.5°C and a pressure of 1.10 atm?