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4. If one starts with pure NO2(g) at a pressure of 0.500 atm, the total pressure inside the reaction vessel when 2NO2(g) 2NO(g) + O2(g) reaches equilibrium is 0.674 atm. Calculate the equilibrium partial pressure of NO2.


A. 0.152 atm
B. 0.174 atm
C. 0.200 atm
D. 0.326 atm
E. The total pressure cannot be calculated because Kp is not given.

5. For the reaction H2(g) + I2(g) 2HI(g), Kc = 50.2 at 445ºC. If [H2] = [I2] = [HI] = 1.75 ´ 10-3 M at 445ºC, which one of these statements is true?


A. The system is at equilibrium, thus no concentration changes will occur.
B. The concentrations of HI and I2 will increase as the system approaches equilibrium.
C. The concentration of HI will increase as the system approaches equilibrium.
D. The concentrations of H2 and HI will fall as the system moves toward equilibrium.
E. The concentrations of H2 and I2 will increase as the system approaches equilibrium.