So we have substances in different phases. Oxide and carbon dioxide, calcium carbonate is a solidĪnd calcium oxide is a solid, but carbon dioxide is a gas.
Of calcium carbonate to turn into calcium In different phases, we call it a heterogeneous equilibrium. Reactants and products are in the same phase, we call this a homogeneous equilibrium. For the synthesis of ammonia, everything was in the gaseous state. Times the partial pressure of hydrogen raised to the third power. Pressure of nitrogen raised to the first power Pressure of our product, ammonia, raised to the second power divided by the partial So we would write Kp is equal to, we think about products over reactants. So if we go back to our previous reaction where everything was in the gaseous state, we could write a Kp expression. And Kc and Kp usually haveĭifferent values from each other. And if we did that, instead of writing Kc, we would write Kp where We could write an equilibriumĬonstant expression using partial pressures So let's say that A, B,Ĭ and D are all gases. For gases, it's often more convenient to measure partial pressures instead of measuring concentrations. And because there's a coefficient of three in the balanced equation, we raise the concentration of Of our other reactants, which is hydrogens. Of nitrogen to the first power multiplied by the concentration One in the balanced equation, that'd be the concentration So we write the concentration of nitrogen. So we write the concentration of ammonia and we raise the concentration of ammonia to the power of the coefficient in the balanced equation, which is a two. With concentrations, and we start with our We start by writing theĮquilibrium constant Kc, c because we're dealing Let's write an equilibriumĬonstant expression for the following reaction, which shows the synthesis of ammonia from nitrogen and hydrogen, and everything is in the gaseous state. And K is constant forĪ particular reaction at a certain temperature. And when we plug in ourĮquilibrium concentrations into our equilibrium constant expression, we get a value for theĮquilibrium constant K. That the concentrations that we're plugging into our equilibrium constant expression are equilibrium concentrations. Of the two reactants multiplied by each otherĪnd raised to the power, each concentration is raised to the power of the coefficient in In the denominator, we have the concentrations And the concentration of each product is raised to the power of the coefficient. Have the concentrations of our two products multiplied together. And the equilibriumĬonstant Kc is equal to, and in the numerator, we If we were to write anĮquilibrium constant expression for this hypothetical reaction, we'd start by writing theĮquilibrium constant K and then we have a subscript c here because we're dealing with concentrations in our equilibrium constant expression. So we have a lowercase a, a lowercase b, lowercase c and lowercaseĭ as coefficients in our balanced equation. And in the balanced equation, the lowercase lettersĪre the coefficients. Let's say we have a hypothetical reaction where reactants A and B Constant is symbolized by the letter K, andĮquilibrium constant tells us about the relativeĬoncentrations of reactants and products at equilibrium.
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