Calculate Kp at 500 deg C for the reaction- 4No2+6H2O <---> 4NH3+5O2. The value for Kc at 500 deg C is equal to 0.456.
Kc = KpRT-delta n
where delta n = ngas products - ngas reactants
To calculate Kp at 500 deg C for the given reaction, we need to find the value of Kp using the equation Kc = KpRT^(-Δn), where Kc is the given value of Kc at 500 deg C, R is the gas constant, T is the temperature in Kelvin, and Δn is the difference in the number of moles of gaseous products and gaseous reactants.
First, we need to determine the Δn for the reaction:
Δn = (n_gas products) - (n_gas reactants)
From the balanced equation, we can see that there are 4 moles of NH3 and 5 moles of O2 as gaseous products, while there are 4 moles of NO2 and 6 moles of H2O as gaseous reactants.
So, Δn = (4+5) - (4+6) = 3 - 10 = -7
Now, we have all the values needed to calculate Kp:
T = 500 deg C = 500 + 273 = 773 K (converted to Kelvin)
Kc = 0.456
Substituting the values into the equation Kc = KpRT^(-Δn), we get:
0.456 = Kp * R * (773)^(-(-7))
0.456 = Kp * R * (773)^7
To solve for Kp, we need to know the value of the gas constant, R. The gas constant is typically expressed in units of J/(mol·K) with a value of approximately 8.314 J/(mol·K).
So, with the appropriate value of R, we can rearrange the equation to solve for Kp:
Kp = 0.456 / (R * (773)^7)
Plug in the known values for R and calculate Kp.
Note: The units used for Kp will depend on the units used for R. It is essential to ensure that all values used in calculations are in consistent units to obtain accurate results.