1 / 10

Chemical Equations

Chemical Equations. General Chemistry Jim Thorpe High School. Oh, no… Vocabulary!. Coefficient: is a small, whole number that appears IN FRONT of a chemical formula in a chemical equation. Example: 4 HCl Word Equation:

gay-mcintyre
Download Presentation

Chemical Equations

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Chemical Equations General Chemistry Jim Thorpe High School

  2. Oh, no… Vocabulary! • Coefficient: is a small, whole number that appears IN FRONT of a chemical formula in a chemical equation. • Example: 4 HCl • Word Equation: an equation in which the reactants and products in a chemical reaction are represented by words. • Example: hydrogen + oxygen yields water • Formula Equation: represents the reactants and products of a chemical reaction by their symbols or formulas. • Example: 2 H2 + O2 2 H2O

  3. Why are we learning this? • The coefficients of a chemical reaction indicate relative amounts of reactants and products. Coefficients are MOLE RATIOS Example: H2(g) + Cl2(g)  2HCl(g) 1 mol H2 : 1 mol Cl2 : 2 moles HCl • The relative masses of the reactants and products can also be determined from the coefficients. Example: 1 mol H2 = 2.02 g H2 1 mol Cl2 = 70.90 g Cl2 2 mol HCl = 72.92 g HCl Therefore, 2.02g H2 will react with 70.90g Cl2 to form 72.92g of HCl.

  4. The reverse reaction for a chemical equation has the same relative amounts of substances as the forward reaction. So what? Because of this, chemical reactions can be read in any direction. Forward and Reverse.

  5. Ahh…not another note card! Symbols used in Chemical Equations • Open your books to page 246. • Tonight cut out 13 flashcards. • On the front of each card, draw the symbol. • On the back, write its explanation. • When you are finished, find a partner and practice!

  6. Law of Conservation of Mass The law of conservation of mass states that matter is neither lost nor gained in chemical reactions. It simply changes form.

  7. Atoms are indestructible and unchangeable, so compounds are formed when one atom chemically combines with other atoms. When elements react to form compounds, they react in defined, whole-number ratios. Reactions are not random events. They proceed according to precise and well-defined formulas. Dalton’s Law of Definite Proportions

  8. Write a word equation. Determine the reactants, the products, and the physical states involved. Translate to Chemistry. Write the unbalanced equation that summarizes the reaction described in Step 1, using chemical formulas for names. Solid zinc and hydrochloric acid react to yield zinc chloride and hydrogen gas. Zn(s) + HCl  ZnCl2 + H2(g) Rules for Balancing Equations

  9. Satisfy the law of conservation of mass. Start with the most complicated molecule. Determine the coefficients necessary to satisfy the law of conservation of mass. Check your work. 3. Zn(s) + HCl  ZnCl2 + H2(g) __Zn(s) + __HCl  1 ZnCl2 + __H2(g) 1 Zn(s) + 2 HCl  1 ZnCl2 + __H2(g) 1 Zn(s) + 2 HCl  1 ZnCl2 + 1 H2(g) 4. 1 Zn, 2 H, 2 Cl  1 Zn, 2 H, 2 Cl Rules for Balancing Equations

  10. Examples: __Al + __O2 __Al2O2 __C2H6 + __O2 __CO2 + __H2O __Fe2O3 + __H2SO4 __Fe2(SO4)3 + __H2O

More Related