A flask is charged with 1.540 atm of N2O4(g) and 0.97 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below. N2O4(g) 2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4?
A flask is charged with 1.540 atm of N2O4(g) and 0.97 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below. N2O4(g) 2NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4?
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A flask is charged with 1.540 atm of N2O4(g) and 0.97 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.
N2O4(g) 2NO2(g)
After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.(a) What is the equilibrium partial pressure of N2O4?
atm
(b) Calculate the value of Kp for the reaction.
(c) Is there sufficient information to calculate Kcfor the reaction?
No, because the value of Kc can be determined experimentally only.Yes, because the partial pressures of all the reactants and products are specified. Yes, because the temperature is specified.
If Kc can be calculated, find the value of Kc. Otherwise, enter 0.
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