Determine the values of Kp that correspond to the following values of Kc
a)CO(g) + Cl2(g) <===> COCl2(g)
Kc= 1.2 x 10^3 at 668 K
b)2 NO(g)+ Br2(g)<===> 2 NOBr(g)
Kc= 1.32 x 10^-2 at 1000 K
c) 2 COF2(g)<===> CO2(g)+ CF4(g)
Kc= 2.00 at 1000 degrees Celsius
Kp = Kc*R*Tdelta n
where delta n = n(products)-n(reactants).
Kp = 1.2E3*0.08206*(1-2) = ??
The others follow the same pattern.
Help me
To determine the values of Kp that correspond to the given values of Kc, you need to use the relationship between Kc and Kp, which is based on the ideal gas law.
The equation relating Kp and Kc is as follows:
Kp = Kc * (RT)^(Δn)
Where:
Kp is the equilibrium constant in terms of partial pressures.
Kc is the equilibrium constant in terms of molar concentrations.
R is the gas constant (0.0821 L·atm/(mol·K)).
T is the temperature in Kelvin.
Δn is the difference in the number of moles of gaseous products and the number of moles of gaseous reactants.
Let's use this equation to determine the values of Kp for each given value of Kc.
a) For the reaction CO(g) + Cl2(g) <===> COCl2(g), Kc = 1.2 x 10^3 at 668 K.
First, we need to determine the value of Δn. In this case, Δn = (1+1) - 1 = 1, because there is one mole of gaseous product and one mole of gaseous reactant.
Now, substitute the values into the equation:
Kp = (1.2 x 10^3) * (0.0821 L·atm/(mol·K))^(1) * 668 K
Simplify the expression and calculate the value of Kp.
Kp ≈ 96.73
b) For the reaction 2 NO(g) + Br2(g) <===> 2 NOBr(g), Kc = 1.32 x 10^-2 at 1000 K.
Again, we need to determine the value of Δn. In this case, Δn = (2+1) - 2 = 1, because there are two moles of gaseous products and two moles of gaseous reactants.
Now, substitute the values into the equation:
Kp = (1.32 x 10^-2) * (0.0821 L·atm/(mol·K))^(1) * 1000 K
Simplify the expression and calculate the value of Kp.
Kp ≈ 0.102
c) For the reaction 2 COF2(g) <===> CO2(g) + CF4(g), Kc = 2.00 at 1000 degrees Celsius.
In this case, we need to convert the temperature from Celsius to Kelvin by adding 273 to the given value.
T = 1000 + 273 = 1273 K
Now, we need to determine the value of Δn. In this case, Δn = (1+1) - 2 = 0, because there are equal moles of gaseous products and gaseous reactants.
Now, substitute the values into the equation:
Kp = (2.00) * (0.0821 L·atm/(mol·K))^(0) * 1273 K
Simplify the expression and calculate the value of Kp.
Kp ≈ 2.00
Therefore, the values of Kp that correspond to the given values of Kc are approximately 96.73 (for part a), 0.102 (for part b), and 2.00 (for part c).