(Solved): need help with both parts please!! \pm Pressure-Based versus Concentration-Based Equilibrium Constan ...

\pm Pressure-Based versus Concentration-Based Equilibrium Constants The equilibrium constant, $$K_c$$, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, $$K_p$$, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation $$K_{\mathrm{p}}=K_{\mathrm{c}}(RT{)}^{?n}$$ where $$R=0.08206\mathrm{L}?\mathrm{atm}/(\mathrm{K}?\mathrm{mol}),T$$ is the absolute temperature, and $$?n$$ is the change in the number of moles of gas (sum moles products - sum moles reactants). For example, consider the reaction $${\mathrm{N}}_2(\mathrm{g})+3{\mathrm{H}}_2(\mathrm{g})?2{\mathrm{NH}}_3(\mathrm{g})$$ for which $$?n=2?(1+3)=?2$$. For the reaction $$3\mathrm{A}(\mathrm{g})+2\mathrm{B}(\mathrm{g})?\mathrm{C}(\mathrm{g})$$ $$K_c=30.8$$ at a temperature of $$153{}^{?}\mathrm{C}$$. Calculate the value of $$K_{\mathrm{p}}$$. Express your answer numerically. Part B For the reaction $$X(\mathrm{g})+2Y(\mathrm{g})?3Z(\mathrm{g})$$ $$K_{\mathrm{p}}=275\times 10^{?2}\text{ at a temperature of }231^{?}\mathrm{C}$$ Calculate the value of $$K_{\mathrm{c}}$$ Express your answer numerically.