Chem 1211 1st Edition Lecture 7 Outline of Last Lecture I. Percent CompositionII. Formulas from Elemental Composition Outline of Current Lecture I. Balancing EquationsCurrent LectureI. Balancing Equationsa. ConcepTest: For this reaction that describes a steelmaking process (a)Fe2O3 + (b)C (c)Fe + (d)CO2, which coefficients represent the balanced equation?i. Answer: a=2, b=3, c=4, d=3b. ConcepTest: For the reaction P4 + 6 Cl2 2 PCl3, in which the product begins to burn, what went wrong?i. Answer: Nothing went wrong… the reaction occurred, and it gave off enough heat to ignite c. ConcepTest: For this reaction that describes a steelmaking process, 2 Fe2O3 + 3 C 4 Fe +3 CO2, what percentage of the mass of the products escapes to the atmosphere? i. Answer: 37%ii. Reasoning: The total mass of the products is (4 x mass of Fe) + (3 x mass of C) + (6 x mass of O) = 355.4g. 1. The part of the product that escapes to the atmosphere is 3 CO2; take the total mass of 3 CO2 and divide it by the total mass of the products.2. This gives you .37; multiply by 100 to get the percentage, and the answer is 37%d. Law of Conservation of Massi. Matter is not created or destroyedii. Balanced chemical equationsiii. Formulated by Antoine Lavoisier in 1789e. ConcepTest: This reaction describes the formation of ammonia: 2H2 + N2 2 NH3. At equilibrium, which of the following are TRUE?These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.i. Three H2 and one N2 are required to form each NH3ii. Some H2 and N2 still exist as those moleculesiii. Some NH3 is reverting back to H2 and N21. Answer: ii and iii (this is a equilibrium
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