The equilibrium constant for the chemical equation is Kp = 24.6 at 181 �C. Calculate the...

The equilibrium constant for the chemical equation is Kp = 24.6 at 181 �C. Calculate the value of the Kc for the reaction at 181 �C.

N2 (g) + 3H2 (g) ---> 2NH3 (g)

K_c = ?

Expert Solution

queen_honey_blossom answered 2 years ago

1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K calculate the equilibrium...

1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PPCl5 = 0.610 atm, PPCl3 = 0.400 atm and PCl2 = 0.000 atm. PPCl5 = PPCl3 = PCl2 = 2. H2O(g) + Cl2O(g) <-----> 2HClO(g) Kc = 0.14 at 298.15 K calculate the equilibrium concentrations of the reactants and products if the initial concentrations are [H2O(g)] = 0.00482 mol L-1, [Cl2O(g)] = 0.00482...

a. Calculate the equilibrium constant Kp for the dissociation of dinitrogen tetroxide at 25c: N2O4 =...

a. Calculate the equilibrium constant Kp for the dissociation of dinitrogen tetroxide at 25c: N2O4 = 2NO2 Given Delta H of rxn = 57.20 kJ/mol b. What is the value of Kp at 55c? c. Calculate the degree of dissociation (alpha) of N2O4 at 55c with a pressure of 1.000 bar. The quantity of alpha is defined as the fraction of dimer molecules that have dissociated. Delta G of formation for N2O4= 97.787 kJ/mol Delta G of formation for NO2...

Be sure to answer all parts. At 430 ° C, the equilibrium constant (KP) for the...

Be sure to answer all parts. At 430 ° C, the equilibrium constant (KP) for the reaction 2NO(g) + O2(g) ⇆ 2NO2(g) is 1.5 × 105. In one experiment, the initial pressures of NO, O2, and NO2 are 7.4 × 10−3 atm, 4.2 × 10−2 atm, and 0.20 atm, respectively. Calculate QP and predict the direction that the net reaction will shift to reach equilibrium. What is QP for the experiment? In which direction will the system proceed to reach equilibrium?...

At a certain temperature, the equilibrium constant for the following chemical equation is 3.40. At this...

At a certain temperature, the equilibrium constant for the following chemical equation is 3.40. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.53 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.

At a certain temperature, the equilibrium constant for the following chemical equation is 2.20. At this...

At a certain temperature, the equilibrium constant for the following chemical equation is 2.20. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.73 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium.

At a certain temperature, the equilibrium constant for the following chemical equation is 4.00. At this...

At a certain temperature, the equilibrium constant for the following chemical equation is 4.00. At this temperature, calculate the molarity (M) of NO2(g) that must be added to a starting concentration of 2.73 M SO2(g) (with no products initially present) in order to have formed 1.30 M SO3(g) and 1.30 M NO(g) when equilibrium is reached. SO2(g)+NO2(g)−⇀↽−SO3(g)+NO(g) molarity =

Calculate the value of Kp for the equation. C(s) + CO2(g) 2CO(g) Kp=? Given that at...

Calculate the value of Kp for the equation. C(s) + CO2(g) 2CO(g) Kp=? Given that at a certain temperature: C(s) + 2H2O(g) CO2(g) + 2H2(g) Kp1= 3.53 H2(g) + CO2(g) H2O(g) + CO(g) Kp2 = 0.699 Kp=?????

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on (a) total pressure (b) catalyst used (c) amount of H2 and I2 (d) temperature

In chemical equation H2 (g) + I2 (g) ⇌ 2HI (g) the equilibrium constant Kp depends on___________.(a) total pressure(b) catalyst used(c) amount of H2 and I2(d) temperature

At a certain temperature, the equilibrium constant for the following chemical equation is 3.20. SO2 (g)...

At a certain temperature, the equilibrium constant for the following chemical equation is 3.20. SO2 (g) + NO2 (g) ⇌ SO3 (g) + NO (g) At this temperature, calculate the number of moles of NO2(g) that must be added to 2.40 mol of SO2(g) in order to form 1.00 mol of SO3(g) at equilibrium.

At a certain temperature, the equilibrium constant for the following chemical equation is 2.50. SO2(g) +...

At a certain temperature, the equilibrium constant for the following chemical equation is 2.50. SO2(g) + NO2(g)<---> SO3(g) + NO(g) At this temperature, calculate the number of moles of NO2(g) that must be added to 2.86 mol of SO2(g) in order to form 1.30 mol of SO3(g) at equilibrium. Solve for the number of moles for NO2

Question