Calculate Kc for each reaction. b. N2(g) + O2(g) ⇌ 2 NO(g) Kp = 4.10×10^–31 (at 298 K)

Video transcript

Welcome back everyone to another video. Calculate KC for each reaction B methane gas reacts with water vapor and they produce carbon monoxide gas and three moles of hydrogen gas. The KP of this reaction is equal to 2.5 multiplied by 10 of the third at 1200 Kelvin. And we are given three, sorry for answer choices. A is 2.5 multiplied by 10 of the third B 0.26 C 0.84 and D 1.2 multiplied by 10 of the 13 power. Now, first of all, what we want to understand in this problem is that we can use the relationship between KC and KP. Let's recall that KC is equal to KP divided by RT, erase the power of delta M. And soon we will understand the meaning of each variable. So first of all KP is the equilibrium constant in terms of partial pressures. And it is already given to us, we can simply put 2.5 multiplied by 10 of the third. Now, on the bottom, we can start with R which is the universal gas constant. And here we use 0.08 to 0 6 L multiplied by atmospheres, divided by mole multiplied by Kelvin. Those are the units that we want to use. Now, temperature is the absolute temperature given to us that's 1200 Kelvin. And finally, delta N is the change in the number of moles of gasses in our reaction. So on the right hand side, we have one mole of co and three moles of age two. So take one plus three and we need to subtract the sum. On the left hand side, we have one mole of methane and one mole of water. So in this case, delta M would be four minus two, which gives us two. So we're using a square and when we perform the calculation, we end up with 0.26. So this is the equilibrium constant in terms of molarity. And we can essentially state that the correct answer choice to this problem would be B Thank you for watching.