At a given temperature Kc=1.69 for the reaction: H_2(g) + CO_2(g) leftrightarrow

Question

At a given temperature Kc=1.69 for the reaction: H_2(g) + CO_2(g) leftrightarrow H_2O_(g) + CO_(g) If 0.40 mole of H_2 and 0.40 mole of CO_2 are placed in a 1.0-L container at this temperature, the equilibrium concentration of water will be: If the equilibrium, P_4(g) + 6 Cl_2(g) leftrightarrow 4 PCl_3(g) Is established by adding equal numbers of moles of P_4 and Cl_2 to an evacuated flask, which of the following must be true at equilibrium? [Cl_2] > [PCI_3] [Cl_2] > [P_4] [PCI_3] > [P_4] [P_4] > [CI_2] [P_4] > [PCI_3] 2.0 moles of ammonia are introduced into a 1.0-L container in which it partially dissociates at high temperatures: 2 NH_3(g) leftrightarrow H_2(g) + N_2(g) At equilibrium at a particular temperature 1.0 mole of ammonia remains. K_c is:

Explanation / Answer

5) H2 + CO2 <-----> H2O + CO

Kc = [H2O][CO]/[H2][CO2]

1.69 = (X^2/((0.4-X)(0.4-X)))

X = 0.226 mol

[H2O] = 0.226 M

[CO] = 0.226 M

6) ANSWER: D

7) 2NH3 ----> N2 + 3H2

   kC = [n2][h2]^3/[nh3]^2

      = (1.5^3*0.5/1^2)

    = 1.6875

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