Excess solid P 4 is placed in a0.500 L flask of air at 298 K and 1.000 atm. The

Question

Excess solid P4 is placed in a0.500 L flask of air at 298 K and 1.000 atm. The flask is sealedand the P4 reactswith the oxygen in the air mixture. The pressure in the flask dropsfrom 1.000 atm to 0.791 atm during the reaction. Assume constanttemperature for this process.
The molar mass of P4 = 123.89 g/mol.
P4 (s) + 5O2(g) --> P4O10(s)
What mass of P4reacted?
Thank you in advance!!
The molar mass of P4 = 123.89 g/mol.
P4 (s) + 5O2(g) --> P4O10(s)
What mass of P4reacted?
Thank you in advance!! What mass of P4reacted?
Thank you in advance!!

Explanation / Answer

I realize the mistake I made. I calculated for moles ofP4, however since it is a solid, it cannot be calculatedusing the ideal gas equation. Therefore, PV = nRT (1.000 atm)(0.500 L) = n(0.08206 L atm/mol K)(298 K) n = 0.0204 mol O2 initially PV = nRT (0.791 atm)(0.500 L) = n(0.08206 L atm/mol K)(298 K) n = 0.0162 mol O2 left after reaction 0.0204 - 0.0162 = 0.0042 mol O2 reacted Now use stoichiometry to find the mass of P4 required toreact with 0.0042 mol O2. 0.0042 mol O2 x 1 mol P4 x 123.89 g P4 = 0.104 gP4                           5 mol O2      mol P4

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