Given the reaction: P4(l) + 6 Cl2(g) → 4 PCl3(l) If the percent yield is 82%, what mass of P4 is required to obtain 2.30 g PCl3 (Cl2 in excess)?
_____ g
Given the reaction: P4(l) + 6 Cl2(g) → 4 PCl3(l) If the percent yield is 82%,...
The percent yield for the reaction PCl3 + Cl2 → PCl5 is 85.0 percent. What mass of PCl5 would be expected from the reaction of 60.7 grams of PCl3 with excess chlorine?
The percent yield for the reaction PCl3 + Cl2 → PCl5 is 62.9 percent. What mass of PCl5 would be expected from the reaction of 30.1 grams of PCl3 with excess chlorine?
The percent yield for the reaction PCl3 + Cl2 → PCl5 is 82.2 percent. What mass of PCl5 would be expected from the reaction of 34.4 grams of PCl3 with excess chlorine?
Given: PCl5(s) → PCl3(g) + Cl2(g) ΔH°rxn = + 157 kJ P4(g) + 6 Cl2(g) → 4 PCl3(g) ΔH°rxn = - 1207 kJ What is the standard-state enthalpy change for the following reaction? P4(g) + 10 Cl2(g) → 4PCl5(s)a -2100 kJb-1835 kJc-1364 kJD -1786 kJ
Use the standard reaction enthalpies given below to determine H°rxn for the following reaction: P4 (g) + 10 Cl2 (g) --> 4 PCl5 (s) ΔHreaction = ? Given: PCl5 (s) --> PCl3 (g) + Cl2 (g) ΔHreaction = +157 kJ P4 (g) + 6 Cl2 (g) --> 4 PCl3 (g) ΔHreaction = -1207 kJ Choices: A. -1835 kJ B. -1364 kJ C. -1050 kJ D. -1786 kJ E. -2100 kJ
Assume the reaction of 118.30 g of P4 in the following reaction to determine the other quantities. 1P4 + 6Cl2 -> 4PCl3 moles of P4 reacting = mol moles of Cl2 required = mol moles of PCl3 formed = mol mass of PCl3 formed = g
Assume the reaction of 60.63 g of Cl2 in the following reaction to determine the other quantities. 6Cl2 + 1P4 -> 4PCl3 moles of Cl2 reacting = ____mol moles of P4 required = _____mol moles of PCl3 formed = _____mol mass of PCl3 formed = ______ g
4. (10 points)Given the following data: P4 (s) + 6 Cl2 (g) -------> 4 PC13 (1) P4 (8) + 10 Cl2 (g) -------> 4 PCls (g) AG° = -1088 kJ/mole P4 AG° = -1292 kJ/mole P4 Calculate AGº for the reaction PC13 (1) + Cl2 (g) -------> PCI; (g) (answer only 1 point)
Phosphorous pentachloride decomposes according to the reaction PCl5(g)↽−−⇀PCl3(g)+Cl2(g)PCl5(g)↽−−⇀PCl3(g)+Cl2(g) A 13.5 g13.5 g sample of PCl5PCl5 is added to a sealed 1.50 L1.50 L flask and the reaction is allowed to come to equilibrium at a constant temperature. At equilibrium, 34.8%34.8% of the PCl5PCl5 remains. What is the equilibrium constant, ?cKc , for the reaction? ?c=Kc=
The equilibrium constant Kc for the reaction: PCl3(g) + Cl2(g) PCl5(g) is 490 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established? (show work)