Calculate K c for each reaction. b. CH 4 (g) + H 2 O(g) ⇌ CO(g) + 3 H 2 (g) K p = 7.7x10 24 (at 298 K) c. I 2 (g) + Cl 2 (g) ⇌ 2 ICl(g) K p = 81.9 (at 298 K)

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.

Ch.15 - Chemical Equilibrium

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Tro 4th Edition

Ch.15 - Chemical Equilibrium

Problem 31b,c

Chapter 15, Problem 31b,c

Calculate K_c for each reaction.
b. CH₄(g) + H₂O(g) ⇌ CO(g) + 3 H₂(g) K_p = 7.7x10²⁴ (at 298 K)
c. I₂(g) + Cl₂(g) ⇌ 2 ICl(g) K_p = 81.9 (at 298 K)

Verified step by step guidance

Identify the relationship between Kc and Kp using the equation: Kc = Kp(RT)^-Δn, where R is the ideal gas constant (0.0821 L·atm/mol·K) and T is the temperature in Kelvin.

Determine Δn, the change in moles of gas, by subtracting the sum of the moles of gaseous reactants from the sum of the moles of gaseous products. For the given reaction, Δn = (1 + 3) - (1 + 1).

Substitute the given values into the equation: Kc = 7.7x10^24 * (0.0821 * 298)^-Δn.

Calculate the value of (RT)^-Δn using the values of R, T, and Δn.

Multiply Kp by the calculated value of (RT)^-Δn to find Kc.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Equilibrium Constant (Kc and Kp)

The equilibrium constant (K) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction. Kc refers to concentrations in molarity, while Kp refers to partial pressures. The relationship between Kc and Kp is given by the equation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. Understanding this relationship is crucial for converting between Kc and Kp.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in a reaction, not just at equilibrium. It is calculated using the same formula as K, but with the current concentrations or pressures. Comparing Q to K helps predict the direction in which a reaction will proceed to reach equilibrium, which is essential for understanding dynamic chemical systems.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is disturbed by changes in concentration, temperature, or pressure, the system will adjust to counteract the disturbance and restore a new equilibrium. This principle is vital for predicting how changes in conditions will affect the position of equilibrium and the values of Kc and Kp in a given reaction.