7. (a) If the partial pressure of each component is 1 atm, and the temperature is...
At a particular temperature, Kp-0.39 for the reaction below. N204(g) 2 NO2(g) (a) A flask containing only N204 at an initial pressure of 4.8 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. N2O4 NO2 atm (b) A flask containing only NO2 at an initial pressure of 9.6 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. No2 (e) From your answers to parts (e) and (b), does it matter...
At a certain temperature and total pressure of 1.2 atm. the partial pressures of an equilibrium mixture for 2A(g) B(g) are P_A - 0.60 atm and P_B - 0.60 aim. After a disturbance, the system regains equilibrium with a total pressure of 1.6 atm. What is the partial pressure of A at the equilibrium ? atm
1) At 298 K, an equilibrium mixture contains P H2=0.958 atm, P I2= 0.877 atm and P HI=0.020 atm. Please try and answer all! You must show all your work to receive credit. Watch sig figs! Consider the reaction: 1) At 298 K, an equilibrium mixture contains P H2-0.958 atm, P ½=0.877 atm, and P HI-0.020 atm. Calculate the value of the equilibrium constant Kp? a) (o, o2) 0.938x o.87? b) And what is the value of the equilibrium constant...
A flask containing only N204 at an initial pressure of 4.5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the two gases, given Kp 0.25 at a particular temperature for the following reaction. Show your work in the space provided. 3. Noode) 2 NO2(g)
Consider the gas phase reaction 302(g) 203(g) (a) At 298K and a total pressure of 1 atm, what are the partial pressures at equilibrium? (b) What about at 398K and a total pressure of 1 atm? 3.
Consider the gas phase reaction 302(g) = 203(g). (a) At 298K and a total pressure of 1 atm, what are the partial pressures at equilibrium? (b) What about at 398K and a total pressure of 1 atm?
A mixture of He, Ar, and Xe has a total pressure of 2.80 atm . The partial pressure of He is 0.300 atm , and the partial pressure of Ar is 0.300 atm . What is the partial pressure of Xe? A volume of 18.0 L contains a mixture of 0.250 mole N2 , 0.250 mole O2 , and an unknown quantity of He. The temperature of the mixture is 0 ∘C , and the total pressure is 1.00 atm...
Determine the partial pressures of NO2(g) and N2O4(g) inside the cylinder assuming both gases are ideal. 2) (20 points) A piston-cylinder arrangement contains a mixture of NO2(g) and N204(g) which are in chemical equilibrium at 298K. Kp=6.739 at this temperature. If the piston is adjusted so as to make the total pressure inside the cylinder equal to 2bar, determine the partial pressures of NO2(g) and N204(g) inside the cylinder assuming both gases are ideal. How can you verify your answers?...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g) + 3H2(g) + 2NH3(g) the standard change in Gibbs free energy is AG° –72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are Pin, 0.150 atm, PH, = 0.200 atm, and PNH, 0.850 atm? = = =
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) the standard change in Gibbs free energy is Δ?°=−72.6 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.500 atm , ?O2=0.400 atm , and ?NO2=0.750 atm ?