1. The balanced chemical equation for the reaction is:
2NO(g) + O2(g) -> 2NO2(g)
2. Let x be the change in concentration from the initial moles for NO2. The equilibrium concentrations are:
[NO] = 4 - 2x mol/L
[O2] = 2.5 - x mol/L
[NO2] = x mol/L
3. A positive enthalpy change indicates an endothermic reaction. Therefore, increasing the temperature would favor the formation of products, so the reaction would proceed to the right.
4. If the volume of the product NO2 is increased, the equilibrium will shift to the right in order to balance the new conditions. This is because the system will try to reduce the effect of the volume change by favoring the side with more moles of gas.
5. If the temperature is increased, the equilibrium constant (Kc) value will also increase. This is due to Le Chatelier's principle, as the system will shift the equilibrium to oppose the increase in temperature.
6. If the concentration of Nitrogen oxide (NO) were increased, the equilibrium would shift to the left to consume the excess NO and produce more NO2 until a new equilibrium is established.
7. If Kc was greater than the Reactant Quotient (Qc), the reaction would proceed in the reverse direction until Qc equals Kc and equilibrium is reestablished.
8. To calculate Kp, you can use the equation: Kp = Kc(RT)^Δn, where R is the ideal gas constant (0.0821 L*atm/mol*K) and Δn is the difference in moles of gas between products and reactants. Given that the reaction is 2NO(g) + O2(g) -> 2NO2(g), Δn = 2 - (1+1) = 0. Therefore, Kp = Kc = 0.001.
In a chemical reaction, 4mol of Nitrogen monoxide (NO) and 2.5mol of Oxygen (O2) are mixed together in a container with a volume of 1000ml to produce Nitrogen Dioxide (NO2).If equilibrium constant (Kc) for this reaction is 0.001.
1. Write a balanced chemical equation for the above reaction?
2. Determine the equilibrium concentrations for each substances ?
3. If the overall enthalpy of the above reaction is 49kJ/mol. Predict the outcome of the reaction?
4. If the volume of the product, NO2 is being increased, where will equilibrium shift to and why will it have to shift that way?
5. What is happen to the equilibrium constant (Kc) value if temperature is increased?
6. If some concentration of Nitrogen oxide (NO) were increased, what would happen to the equilibrium?
7. What would happen to above reaction if we assumed that equilibrium constant (Kc) was greater than Reactant Quotient (Qc)?
8. Calculate it's Kp value if temperature of the reaction is at 25°C?
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