Determine the values of Kc that correspond to the following values of Kp
(a) SO2Cl2(g)--->SO2(g) + Cl2(g)
Kp= 2.9 x 10^-2 at 303 K
(b) 2 NO2 (g)--->2NO(g)+O2(g)
Kp= 0.275 at 700 K
(c)CO(g) + Cl2(g)---> COCl2(g)
Kp= 22.5 at 395 degree Celsius
hello its 7.96*10^-4 ty glhf
Why did the chemist go broke?
Because they couldn't find the right Kc!
But fear not, I'm here to help you determine the values of Kc for these reactions. To do that, we can use the equation:
Kc = Kp(RT)^(delta n)
where Kc is the equilibrium constant in terms of concentrations, Kp is the equilibrium constant in terms of partial pressures, R is the gas constant (0.0821 L·atm/mol·K or 8.314 J/mol·K), T is the temperature in Kelvin, and delta n is the change in the number of moles of gas molecules as the reaction proceeds.
Now let's calculate the values of Kc for each reaction:
(a) SO2Cl2(g) ---> SO2(g) + Cl2(g)
Kp = 2.9 x 10^-2 at 303 K
Here, there is no change in the number of moles of gas molecules, as both sides of the equation have the same number of moles. Therefore, delta n = 0.
Kc = Kp(RT)^0
= Kp
So, Kc = 2.9 x 10^-2.
(b) 2 NO2(g) ---> 2 NO(g) + O2(g)
Kp = 0.275 at 700 K
In this reaction, there is a decrease in the number of moles of gas molecules, as two moles of NO2 form three moles of gas (2 NO + O2). Therefore, delta n = -1.
Kc = Kp(RT)^(-1)
= 0.275(0.0821 L·atm/mol·K)(700 K)^(-1)
= 0.275(0.0821)
= 0.0225
So, Kc = 0.0225.
(c) CO(g) + Cl2(g) ---> COCl2(g)
Kp = 22.5 at 395 degrees Celsius
In this reaction, there is an increase in the number of moles of gas molecules, as one mole of CO and one mole of Cl2 form one mole of COCl2. Therefore, delta n = 1.
First, we need to convert the temperature to Kelvin:
395 degrees Celsius = 395 + 273 = 668 K
Kc = Kp(RT)^(1)
= 22.5(0.0821 L·atm/mol·K)(668 K)^1
= 22.5(0.0821)(668)
= 1007.91
So, Kc = 1007.91.
Voila! We've determined the values of Kc for each reaction. Remember, if you have any more questions or need further assistance, just ask!
To determine the values of Kc corresponding to the given values of Kp, we can use the relationship between Kp and Kc for a gaseous reaction.
The relationship is given by:
Kp = Kc(RT)^(∆ng)
where Kp is the equilibrium constant expressed in terms of partial pressures, Kc is the equilibrium constant expressed in terms of concentrations, R is the gas constant (0.0821 L·atm/(mol·K)), T is the temperature in Kelvin, and ∆ng is the change in the number of moles of gaseous reactants minus the change in the number of moles of gaseous products.
Let's calculate the values of Kc for each reaction:
(a) SO2Cl2(g) ---> SO2(g) + Cl2(g)
Kp = 2.9 x 10^-2 at 303 K
In this reaction, there is no change in the number of moles of gaseous reactants and products (∆ng = 0), so the equation becomes:
Kp = Kc(RT)^0
Kc = Kp / (RT)^0
Kc = Kp
Therefore, the value of Kc corresponding to Kp for this reaction is 2.9 x 10^-2.
(b) 2 NO2(g) ---> 2 NO(g) + O2(g)
Kp = 0.275 at 700 K
In this reaction, there is a decrease of 1 mole of gaseous reactants and an increase of 1 mole of gaseous products (∆ng = 1 - 2 = -1). Let's substitute the values in the equation:
Kp = Kc(RT)^(-∆ng)
0.275 = Kc(RT)^(-(-1))
0.275 = Kc(RT)
To solve for Kc, we need to know the value of T. Once we have this information, we can calculate Kc using the given equation.
(c) CO(g) + Cl2(g) ---> COCl2(g)
Kp = 22.5 at 395 degrees Celsius
In this reaction, there is an increase of 1 mole of gaseous reactants and 1 mole of gaseous products (∆ng = 1 - 1 = 0). Let's substitute the values in the equation:
Kp = Kc(RT)^(∆ng)
22.5 = Kc(RT)^0
22.5 = Kc
Therefore, the value of Kc corresponding to Kp for this reaction is 22.5.
In summary:
(a) Kc = 2.9 x 10^-2
(b) Kc depends on the temperature value, which is not provided.
(c) Kc = 22.5
To determine the values of Kc that correspond to the given values of Kp, we need to use the relationship between Kp and Kc for gaseous reactions. The relationship is given by the equation:
Kp = Kc(RT)^(∆n)
Where:
Kp is the equilibrium constant expressed in terms of partial pressures
Kc is the equilibrium constant expressed in terms of concentrations
R is the gas constant
T is the temperature in kelvin
∆n is the difference in the number of moles of gaseous products and reactants.
To find the values of Kc, we need to determine the ∆n for each reaction and then use the given value of Kp and temperature to solve for Kc.
Let's calculate the values of Kc for each reaction:
(a) SO2Cl2(g) ---> SO2(g) + Cl2(g)
Kp = 2.9 x 10^-2 at 303 K
There are 2 moles of gaseous products and 1 mole of gaseous reactant, so ∆n = (2+1) - 1 = 2
Substituting the values into the equation:
2.9 x 10^-2 = Kc(0.0821 L·atm/(mol·K))(303 K)^(2)
Kc = (2.9 x 10^-2) / (0.0821(303)^2) = 1.27 x 10^-4
Therefore, the value of Kc for the reaction is approximately 1.27 x 10^-4.
(b) 2 NO2(g) ---> 2 NO(g) + O2(g)
Kp = 0.275 at 700 K
There are 3 moles of gaseous products and 2 moles of gaseous reactant, so ∆n = (3+2) - 2 = 3
Substituting the values into the equation:
0.275 = Kc(0.0821 L·atm/(mol·K))(700 K)^(3)
Kc = (0.275) / (0.0821(700)^3) = 1.52 x 10^-7
Therefore, the value of Kc for the reaction is approximately 1.52 x 10^-7.
(c) CO(g) + Cl2(g) ---> COCl2(g)
Kp = 22.5 at 395 degrees Celsius
First, we need to convert the temperature from degrees Celsius to Kelvin:
T = 395 degrees Celsius + 273 = 668 K
There are 1 mole of gaseous product and 2 moles of gaseous reactants, so ∆n = (1+2) - 1 = 2
Substituting the values into the equation:
22.5 = Kc(0.0821 L·atm/(mol·K))(668 K)^(2)
Kc = (22.5) / (0.0821(668)^2) = 1.29 x 10^-4
Therefore, the value of Kc for the reaction is approximately 1.29 x 10^-4.
In summary, the values of Kc that correspond to the given values of Kp are approximately:
(a) 1.27 x 10^-4
(b) 1.52 x 10^-7
(c) 1.29 x 10^-4.