Phosphine (PH3) decomposes at elevated temperatures, yielding gaseous P2 and H2: 2PH3(g)⇌P2(g)+3H2(g) Kp= 398 at 873 K
When a mixture of PH3, P2, and H2 comes to equilibrium at 873 K, PP2= 0.422 atm and PH2= 0.822 atm. What is PPH3?
Phosphine (PH3) decomposes at elevated temperatures, yielding gaseous P2 and H2: 2PH3(g)⇌P2(g)+3H2(g) Kp= 398 at 873...
For the equilibrium 2PH3(g) ⇌ P2(g) +3H2(g), the equilibrium partial pressures are PPH3=0.049 atm, PP2=0.498 atm, and PH2=0.776 atm at 738K. Calculate Kp.
For the reaction H2 S(g) + I2 (s) ⇌ S(s) + 2 HI(g) Kp = 1.33×10–5 at 333 K. What will be the total pressure of the gases above an equilibrium mixture if, at equilibrium, PHI = 0.010 × PH2 S? The answer is 0.134 atm. Please include work and explanation! Thank you :-)
I need pressure and Kp please... a The gas arsine, AsHz, decomposes as follows: 2AsH3(g) = 2As(s) + 3H2(g) In an experiment at a certain temperature, pure AsH3(g) was placed in an empty, rigid, sealed flask at a pressure of 385.0 torr. After 48 hours the pressure in the flask was observed to be constant at 482.0 torr. Calculate the equilibrium pressure of H2(g). Pressure = atm Calculate K, for this reaction. K,=