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41fc8b0a-5b9f-4b45-b149-30d782097e81 Absorbing Summary Taking in, as in a reaction that absorbs heat is endothermic.

306b7857-e276-4b5a-8588-6ced77aa68b8 5. Any reaction or process that consumes heat energy. Endothermic Summary

SABIS Grade 10 T1 W2

a93af1a1-f4ac-4112-9285-fd7aece39636 Soluble Summary The ability of a substance to dissolve in a particular solvent, forming a homogeneous mixture.

b744dd48-89a7-4bbe-bcb3-c584fa0d3ea7 Find heat involved with given # of moles of reactant/product from H Summary Finding the energy supplied by an electric current is crucial in understanding and quantifying electrical energy consumption. The equation commonly used for this purpose is W = IVt, where W represents the energy supplied, I is the current flowing through the circuit, V is the potential difference (voltage) across the circuit, and t is the time for which the current flows. The equation W = IVt is derived from the fundamental relationship between electrical power, current, voltage, and time. Power (P) is defined as the rate at which energy is transferred or consumed, and it can be calculated as the product of current and voltage, P = IV. Multiplying this power by time (t), we obtain the energy supplied or consumed, which is given by the equation W = IVt. To calculate the energy supplied by an electric current, we need to know the values of current (I), voltage (V), and time (t). Current is measured in amperes (A), voltage is measured in volts (V), and time is measured in seconds (s). For example, let's consider a scenario where a circuit has a constant current of 2 amperes (A) flowing through it, a voltage of 12 volts (V) across the circuit, and the current flows for a duration of 10 seconds (s). Using the equation W = IVt, we can calculate the energy supplied as follows: W = (2 A) * (12 V) * (10 s) = 240 joules (J) Therefore, in this case, the energy supplied by the electric current is 240 joules (J). It's important to note that the equation W = IVt assumes that the current and voltage remain constant during the entire time period. In real-world applications, the current and voltage may vary over time, requiring more advanced calculations to determine the total energy supplied.

Lesson 34 Chapter 6 SABIS Grade 10 Part 4 Lesson 34 261. Demonstration: Sublimation: Examples of solids that can sublime at room temperature: 1) Solid iodine, I2 (s) 2) Dry ice or solid carbon dioxide CO2 (s) 3) Any ammonium compound as ammonium chloride, NH4Cl and ammonium bromide, NH4Br 262. Demonstration: Simple Distillation 263. Demonstration: Fractional distillation. Discuss briefly: fractional distillation of liquefied air and fractional distillation of crude oil. 264. Demonstration: Separating funnel 265. Adsorption: means sticking to the surface. 266. Adsorption: sticking of the particles of one material on the surface of another. Examples of adsorbing substances: Silica gel: adsorbs water vapor, Charcoal: adsorbs gases with strong odor and removes colored impurities from a solution 267. Demonstration: Chromatography. It is the technique used to separate different compounds, especially those that can be easily destroyed by heat or chemicals. It can be used to separate colored components as: 1) Green liquid obtained by squashing green leaves. 2) Black ink. The property that carries the liquid up the paper is capillary action. 268. Demonstration: Crystallization 269. Alcohol is flammable, therefore it cannot be heated directly. To heat alcohol, we should use a steam bath or an electric heater. 270. If you need to collect sugar from sugar alcohol solution heat the solution using an electric heater to crystallization point. Leave the solution to cool and crystals to form. Filter off the crystals. 271. Vapor pressure and temperature are proportional NOT directly proportional. At the same temperature, the vapor pressure is the SAME. For the same liquid, the only factor affecting the pressure of the liquid is the temperature. 272. Minimum conditions for liquid molecules to vaporize: 1) Molecules are supposed to be on the surface. 2) Molecules are supposed to have an average kinetic energy greater than the energy keeping the molecules in the liquid state. 273. Water has a vapor pressure of 17.5 mmHg at 20oC. Which of the following will increase the vapor pressure of water? a) Transferring water to a larger container. b) Cooling water to 10oC c) Taking the container to the top of the mountain. d) Heating the water to 32oC 274. Boiling point: is the temperature at which the liquid vaporizes anywhere in the solution. 275. At the boiling point: a. Vapor pressure is equal to the surrounding pressure. b. Bubbles of vapor can form anywhere within the liquid. c. Molecules escape from the surface of the liquid to enter the gas phase as vapor (this also happens at room temperature). d. With increasing altitude, atmospheric pressure decreases and so does boiling point. 276. Normal boiling point: is the temperature at which the vapor pressure is exactly 1 atm or 760 mmHg. 277. Molar heat of fusion: is the energy required to change one mole of a substance from solid to liquid at the same temperature and constant pressure. 278. General equation for Molar heat of vaporization: X (l) + heat ⇌ X (g) 279. General equation for Molar heat of condensation: X (g) ⇌ X (l) + heat 280. In general, a substance that has a higher boiling point is expected to have a 281. An aqueous solution is one in which the solvent is water. 282. Salt and water is an example of aqueous solutions where the solute is a solid. 283. Alcohol and water is an example of aqueous solutions where the solute is a liquid. 284. Ammonia and water is an example of aqueous solutions where the solute is a gas. 285. Concentration: relative amounts of solute and solvent. 286. Molar concentration (Molarity): is the number of moles of solute per liter (dm3) of solution. (the relative amounts of solute and solution) 287. Concentration of a given solution does not change if solution is split into fractions. 288. Relationships between n, V, C and m, M, V, C: n = CV, 𝐂 = 𝐦/𝐕, 𝐕 = 𝐦/𝐂, m = n × M, m = CVM, 𝐌 = 𝐦/𝐂𝐕 289. Preparing solutions with given concentrations. 290. A 2 L bottle of 0.35 M solution is split into ten containers of 100ml capacity. What is the concentration of the solution in each of the new containers? a) 0.75 M b) 0.0035 M c) 2.0 M d) 0.35 M e) 100 M 291. Demonstration: Sublimation: Examples of solids that can sublime at room temperature: 1) Solid iodine, I2 (s) 2) Dry ice or solid carbon dioxide CO2 (s) 3) Any ammonium compound as ammonium chloride, NH4Cl and ammonium bromide, NH4Br 292. Demonstration: Simple Distillation 293. Demonstration: Fractional distillation. Discuss briefly: fractional distillation of liquefied air and fractional distillation of crude oil. 294. Demonstration: Separating funnel 295. Adsorption: means sticking to the surface. 296. Adsorption: sticking of the particles of one material on the surface of another. Examples of adsorbing substances: Silica gel: adsorbs water vapor, Charcoal: adsorbs gases with strong odor and removes colored impurities from a solution 297. Demonstration: Chromatography. It is the technique used to separate different compounds, especially those that can be easily destroyed by heat or chemicals. It can be used to separate colored components as: 1) Green liquid obtained by squashing green leaves. 2) Black ink. The property that carries the liquid up the paper is capillary action. 298. Demonstration: Crystallization 299. Alcohol is flammable, therefore it cannot be heated directly. To heat alcohol, we should use a steam bath or an electric heater. 300. If you need to collect sugar from sugar alcohol solution heat the solution using an electric heater to crystallization point. Leave the solution to cool and crystals to form. Filter off the crystals.

< Back Unit 1 AP Chemistry Topic 5 Periodic Trends You can get more out of your site elements by making them dynamic. To connect this element to content from your collection, select the element and click Connect to Data. Once connected, you can save time by updating your content straight from your collection—no need to open the Editor, or mess with your design. Add any type of content to your collection, such as rich text, images, videos and more, or upload a CSV file. You can also collect and store information from your site visitors using input elements like custom forms and fields. Collaborate on your content across teams by assigning permissions setting custom permissions for every collection. Be sure to click Sync after making changes in a collection, so visitors can see your newest content on your live site. Preview your site to check that all your elements are displaying content from the right collection fields. Ready to publish? Simply click Publish in the top right of the Editor and your changes will appear live. Unit 1 Topic 5 Periodic Trends Previous Next

a58c0537-d56f-4173-bed5-5930eb7a5f15 cheat sheet ap chemistry unit 7 https://k-chemistry.my.canva.site/ap-chemistry-unit-7-cheat-sheet-creation Summary

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574118c5-8840-44df-8b39-f71df47e3da5 6. The process of cooling liquid paradichlorobenzene until it Summary

a29dc9ab-7b50-4705-a143-2732d135dbe8 Alkali metals are very unstable: they react vigorously with O2, Cl2, H2 and water forming stable compounds. Summary

653e3bb2-bc02-474b-8c4f-2f3943af0cde Oxidation Numbers Rules Click the link for the interactive lesson https://examprepnotes.com/oxidation-numbers-lesson-plan Summary