Problem: For the reaction H2(g) + I2(g) ↔ 2 HI(g) At equilibrium‚ the concentrations are found to be [H2] = 0.106 M [I2] = 0.035 M [HI] = 1.29 M What is the equilibrium constant of this reaction? Solution The equilibrium constant (K) for the chemical equation aA + bB ↔ cC + dD can be expressed by the concentrations of A‚B‚C and D at equilibrium by the equation K = [C]c[D]d/[A]a[B]b For this equation‚ there is no dD so it is left out of the equation. K = [C]c/[A]a[B]b
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move away from the surface of the earth‚ such as on the mountains‚ in aeroplanes‚ in spaceships‚ etc. 9. Mass : The amount of matter contained in a body is called mass. It is a scalar quantity and is measured by a physical balance. It is always a constant quantity and its unit in SI system is kilogram. 10. Weight : The force with which a body is attracted towards the centre of the Earth is called weight. O I. VERY SHORT ANSWER QuESTIONS YA Assignments for summAtive Assessment (1 Mark)
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gravitational force between them to observe G‚ the constant of universal gravity that Cavendish investigated. Important Formulas: Procedure: PhET Simulations Play with the Sims Physics Gravity Force Lab 1. Take some time and familiarize yourself with the simulation. Notice how forces change as mass changes and as distance changes. 2. Fill out the chart below for various objects at various distances. 3. Solve for the universal gravitation constant‚ G and compare it to published values. Remember
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Science‚ 3Department of Food Science and Nutrition‚ College of Home Economics‚ University of the Philippines‚ Diliman‚ Quezon City 1101 Philippines ------------------------------------------------- Keywords: forward and reverse reactions‚ equilibrium constant‚ Le Chatelier’s Principle‚ reaction quotient Introduction In chemical kinetics‚ it is stated that a forward reaction’s rate is dependent on the given concentration of the reactants. In other words‚ the relationship of the rate of a reaction is
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algebraically rearranged to pOH = 0.5(pKb + pCb ) 4. K1 = 9.76‚ T1 = 102 K; K2 = 3.74 × 10−61 ‚ T2 = 116 K Explanation: For and endothermic reaction‚ K is directly related to T. For an exothermic reaction‚ K is inversely related to T. K is constant with temperature only for ∆Hrxn = 0 kJ. 002 6.0 points Which combination of ∆G and K is possible? 1. ∆G = −29.4 J‚ K = 1.01 correct 2. ∆G = −77.6 kJ‚ K = 0.981 3. ∆G = 47.3 J‚ K = 3.02 × 1013 4. ∆G = 54.7 kJ‚ K = 1.03 5. ∆G = −82.5 J‚ K =
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the variables mentioned above‚ this experiment was divided into two parts. In Experiment A‚ the radius of the path (length of the string)‚ along with the mass was kept constant‚ and the relation between centripetal force and square of frequency was determined. In Experiment B‚ the Centripetal force and the mass were kept constant‚ and the relationship between square of frequency and the Radius was determined. For Experiment A‚ the results showed that the relationship between the centripetal force
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Chemistry 12 Unit 2 Notes - Equilibrium Chemistry 12 Tutorial 5 – The Equilibrium Constant (Keq) What is Keq ? The "K" in Keq stands for "Constant". The "eq" means that the reaction is at equilibrium. Very roughly‚ Keq tells you the ratio of Products/Reactants for a given reaction at equilibrium at a certain temperature. [Products] [Reactants] K eq = It’s not quite this simple when we deal with real substances. Let’s take an example. It has been found for the reaction: 2HI(g )
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Introduction For this experiment‚ we are going to determine the effect of temperature on solubility‚ to be done in a chemical by dissolving a solute in a definite amount of solution which is saturated. Specifically‚ the goal of this experiment is to prepare a saturated solution of Na2C2O4 in water at different temperatures‚ determine the effect of temperature in solubility‚ and to apply Le Chatelier’s Principle. We can do all this by simply titrating a certain amount of standard KMnO4‚ and measuring
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the state of a reaction when the concentrations of the reactants and products are no longer changing and remain constant. The forward reaction proceeds at the same rate as the reverse reactions making them equal. This type of equilibrium is also named dynamic equilibrium or a dynamic process. When a reaction has reached its chemical equilibrium‚ the constant K value will remain constant unless the temperature changes. If conditions change the concentration in the experiment of any species in the
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place at the same rate. The concentrations of species present remain constant with time. These concentrations are independent of the direction from which equilibrium is approached. The equilibrium constant K is where the partial pressures in atmospheres‚ is a constant‚ independent of the original composition‚ the volume of the container‚ or the total pressure. 12.2 The Equilibrium Constant Expression An equilibrium constant expression can be written for every gaseous chemical system and it states
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