In a chemical reaction 4moles of nitrogen monoxide and 2.5moles of oxygen are mixed together in a container with a volume of 1000ml to produce nitrogen dioxide. If the equilibrium constant for this reaction is 0.001.
1.write the balance chemical equation for the above reaction
2.determine the equilibrium concentration for each of the 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 will happen to the equilibrium constant value if the temperature is increased
6. If some concentration of nitrogen oxide were increased, what would happen to the equilibrium
7. What will happen to the above reaction if we assume that equilibrium constant was greater than reacting quotient
8. Calculate it's Kp value if temperature of the reaction is at 25 degrees Celsius.
1. The balanced chemical equation for the reaction is:
2NO(g) + O2(g) ⇌ 2NO2(g)
2. Let x be the concentration of NO2 produced. Since 2 moles of NO2 is produced for every 2 moles of NO reacted, the equilibrium concentrations of each substance will be:
[NO] = 4 - 2x
[O2] = 2.5 - x
[NO2] = x
3. A positive enthalpy change (+49 kJ/mol) indicates that the reaction is endothermic. Therefore, increasing the temperature will favor the formation of NO2.
4. If the volume of the product NO2 is increased, the equilibrium will shift to the right to counteract the change. This is because by increasing the volume of NO2, the system will try to decrease the concentration of NO2 by favoring the forward reaction.
5. Increasing the temperature will increase the value of the equilibrium constant, as it is an endothermic reaction.
6. If the concentration of nitrogen oxide is increased, the equilibrium will shift to the left to consume the excess reactant, favoring the formation of NO2.
7. If the equilibrium constant is greater than the reacting quotient, the reaction will shift to the right to consume the excess products and reach equilibrium.
8. To calculate the Kp value at 25 degrees Celsius, you will need to know the standard enthalpy change (ΔH°) for the reaction. If the temperature is given in Kelvin, you can use the equation:
ΔG° = -RT ln Kp
ΔG° = ΔH° - TΔS°
Where R = gas constant (8.314 J/mol*K) and ΔS° is the standard entropy change for the reaction.