for the concentrations of the reactants and products. * The equilibrium constant Kc for a reversible reaction is the ratio of the concentrations of the products to the concentrations of the reactants‚ with each concentration raised to the power of their coefficient in the chemical equation. At constant temperature and pressure‚ Kc will remain constant regardless of the concentrations of products and reactants. * The Le Chatelier’s Principle states that any change in concentration‚ partial
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absorptivity‚ the concentration of the substance‚ and the distance the light travels. The Beer Lambert Law states that there is a linear relationship between the concentration of a solution and the absorbance of said solution. If there is a linear relation‚ the resulting graph should be a straight line. If the graph is a straight line‚ this would prove the Beer Lambert Law and fulfill the purpose of this lab. This experiment involves tap water mixed with food colouring but at various concentrations of the solution
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to 12.2g .83% change in mass; the 0.8M bag went from 10.9g to 12.2g and an 11.9% change in mass. During osmosis water diffuses‚ going from an area of low concentration of solute to an area of high concentration of solute. In the case of the lab‚ the area of low concentration of solute was in the beaker‚ and the are of high solute concentration
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moving with or against their concentration gradient in facilitated diffusion? 2. What happened to the rate of facilitated diffusion when the number of carrier proteins was increased? 3. In the simulation you added Na+Cl- to test its effect on glucose diffusion. Explain why there was no effect. Activity 3: 1. Which membrane resulted in the greatest pressure with Na+Cl- as the solute? Why? 2. Explain what happens to the osmotic pressure with increasing solute concentration. 3. If the solutes are
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of Sugars to Soft Drinks Trials Data Collection and Processing: Percentage Transmissions of Light through a Glucose Solution after a Benedicts Treatment | Trial 1 | Trial 2 | Trial 3 | Trial 4 | Trial 5 | Trial 6 | Trial 7 | | Glucose Concentration | Transmission (%)± 0.1 | Transmission (%)± 0.1 | Transmission (%)±0.1 | Transmission (%)± 0.1 | Transmission(%)±0.1 | Transmission (%)±0.1 | Mean (anomalous data not included) ±0.1 | Standard Deviation | 0.00 | 100.0 | 100.0 | 100.0 | 100
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Diffusion & Osmosis: Introduction: This experiment was performed to demonstrate the process of osmosis and to show visible as well as quantitative evidence proving that osmosis occurred. Through the tasks of determining the percent concentrations in two different solutions‚ we were studying the process of osmosis. Osmosis is the best way to perform this experiment because as we went through the experiment‚ the weight of the beaker/dialysis tubing changed and the only logical explanation was
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defined as the movement of water across a semi-permeable membrane from a region of high water concentration to a region of low water concentration. The semi-permeable membrane allows small particles through it but does not allow large particles such as sodium chloride. Osmosis will continue until a state of equilibrium is reached i.e. there is no area with a higher or lower concentration than another area. To land plants‚ water and osmosis are vital as they play leading roles
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substances move down their concentration gradient‚ hence no energy is required. Passive transports can happen through three different channels‚ namely 1. lipid bilayer 2. pore protein 3. carrier protein SIMPLE DIFFUSION What is diffusion? Diffusion is the movement of particles from a high density region to a low density region. No energy is needed and no membrane involves in diffusion. The Dynamic Equilibrium Diffusion will continue until the concentration in all region is the
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data collected on a calibration curve based on concentration and absorbance. We used nitric acid to dissolve a penny to produce another copper (II) nitrate to test its %Transmittance and plot that on the graph to discover the concentration of that substance which came out to be about .21M. We attempted to develop a method for determining the concentration of three different diluted copper (II) ion solutions. We also tried to determine the concentration of copper within a penny by dissolving it in
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equilibrium constant‚ Keq‚ of the Fe3+(aq)+SCN-(aq)↔ FeSCN2+(aq) reaction. By determining the amount of light absorbed‚ the concentration of the colored FeSCN2+ solution was also quantitatively determined. From that data‚ the concentrations of the reagents at equilibrium may also be determined. This experiment should thus provide a Keq value without computing for the concentration of each of the species in the reaction. This experiment will only deal with the aspect of chemical equilibrium‚ particularly
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