Consider the equilibrium of water with gaseous hydrogen and oxygen:
Give the value of for this reaction, if it is written as:
Choose one answer.
a. -7.8 x 10^-16
b. -3.9 x 10^-16
c. 1.3 x 10^-15
d. 6.4 x 10^-14
e. 3.6 x 10^2
3 answers
give the value of WHAT for this reaction, ......
Consider the equilibrium of water with gaseous hydrogen and oxygen:
2H2O(g)=2H2(g) + O2(g) Kp= 7.8x10^-16
Give the value of for this reaction, if it is written as:
1/2O2(g) + H2(g) =H2O(g)
Choose one answer.
a. -7.8 x 10^16
b. -3.9 x 10^16
c. 1.3 x 10^15
d. 6.4 x 10^14
e. 3.6 x 10^7
2H2O(g)=2H2(g) + O2(g) Kp= 7.8x10^-16
Give the value of for this reaction, if it is written as:
1/2O2(g) + H2(g) =H2O(g)
Choose one answer.
a. -7.8 x 10^16
b. -3.9 x 10^16
c. 1.3 x 10^15
d. 6.4 x 10^14
e. 3.6 x 10^7
You still didn't say "of what" but I assume it is Kp after you filled in th remainder of the missing information.
First you turned the reaction around. Let's designate the original Kp as Kp1. That makes the new Kp (which we will call Kp2) = 1/Kp1. THEN you divided all of the coefficients by 2. That makes Kp3 = sqrt(Kp2). Therefore, you take the reciprocal of the original Kp, then take the square root of that.
First you turned the reaction around. Let's designate the original Kp as Kp1. That makes the new Kp (which we will call Kp2) = 1/Kp1. THEN you divided all of the coefficients by 2. That makes Kp3 = sqrt(Kp2). Therefore, you take the reciprocal of the original Kp, then take the square root of that.