(Solved): The reaction N2O42NO2 is allowed to reach equilibrium in a chloroform solution at 25 ...

The reaction $${\mathrm{N}}_2{\mathrm{O}}_4?2{\mathrm{NO}}_2$$ is allowed to reach equilibrium in a chloroform solution at $$25^{?}\mathrm{C}$$. The equilibrium concentrations are $$0.490{\mathrm{mol}}^{\mathrm{L}}{\mathrm{N}}_2{\mathrm{O}}_4$$ and $$2.34\mathrm{mol}/\mathrm{L}{\mathrm{NO}}_2$$. Calculate the equilibrium constant, $$K_{\mathrm{c}}$$, for this reaction. $$K_{\mathrm{c}}=$$ An additional $$1.00\mathrm{mol}{\mathrm{NO}}_2$$ is added to $$1.00\mathrm{L}$$ of the solution and the system is allowed to reach equilibrium again at the same temperature. Select the direction of the equilibrium shift after the $${\mathrm{NO}}_2$$ is added. towards the reactant towards the product no change Determine how the addition of extra $${\mathrm{NO}}_2$$ in the previous step will affect the rate constant, $$K_{\mathrm{c}}$$. $$K_{\mathrm{c}}$$ will increase $$K_c$$ will decrease $$K_c$$ will not change Determine how the addition of extra $${\mathrm{NO}}_2$$ in the previous step will affect the rate constant, $$K_{\mathrm{c}}$$. $$K_{\mathrm{c}}$$ will increase $$K_{\mathrm{c}}$$ will decrease $$K_{\mathrm{c}}$$ will not change Calculate the equilibrium concentrations of $${\mathrm{N}}_2{\mathrm{O}}_4$$ and $${\mathrm{NO}}_2$$ after the extra $$1.00\mathrm{mol}{\mathrm{NO}}_2$$ is added to $$1.00\mathrm{L}$$ of solution. $$\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]$$