Question

How many grams of phosphorus (P4) are needed to completely consume 20.3 L of chlorine gas according to the following reaction at 25 °C and 1 atm?

phosphorus (P4) ( s ) + chlorine ( g ) phosphorus trichloride ( l )

_____ grams phosphorus (P₄)

Answer 1

Answer! Volume occupied by mole of gas at 25°c and I atm condition PV=nRT P = pressure = 1 atm V & Volume=? n & moles = 1 mol T= 25°C+273 = 298 K Re gas constant = 0.0821 Latim moltky : V = nRT imol x 0.0821 Ladmmortkatx 298k Р V I adm N = = 24.46L moles of 2013 L of chlorine. дал 0.83 mol 20:31 X i mol 24.46L . P4 (s) + 642 LG) - 4 P as For 6mol U2 required P4. 1 mol 0.83 mol CO2 required P4 = _ x0.83 mol P4 6 so = 0:138 mol P4 molar mass of Pq = 123.89 g/mol 0138 mol P4 = 0.138 mol X 123.899 i mol 17.1g P4 "please rate it