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Choose from different sets of chemistry matter and change chapter 9 flashcards on Quizlet. Our solutions are written by Chegg experts so you can be assured of the highest quality! For example. Mobile, mountains, ball pen, air, water etc. Q: What are the concentrations of each of the ions in a saturated solution of Pbl2, given that the Ksp of Pbl2 is 8. Download Free PDF. Scott Fogler Eleme. Gabriel Leopoldo. A short summary of this paper.
Solution Manual, Chapter 1 Chapter 1 General: The goal of these problems are to reinforce the definitions and provide an understanding of the mole balances of the different types of reactors. It lays the foundation for step 1 of the algorithm in Chapter 4. This problem might encourage students to get in the habit of writing down what they learned from each chapter.
Small open-ended question from which one could choose one or two parts. Parts a , b or e are recommended. It is straight forward and gives the student an idea of things to come in terms of sizing reactors in chapter 4. SeePl-3 above. This problem can be assigned to just be read and not necessarily to be worked. It will give students a flavor of the top selling chemicals and top chemical companies.
If a reaction occurs, write a balanced equation for the reaction. K is above Zn in the activity series. Cl is below F in the activity series. Fe s Na3PO4 aq 0 No. Fe is below Na in the activity series. Al is above Pb in the activity series. Explain how an activity series of metals is organized. An activity series of metals orders metals by their reactivity with other metals.
The most active metals are on the top of the list, and the least active metals are at the bottom of the list. Compare and contrast single-replacement reactions and double-replacement reactions. AgNO3 aq The two substances at right react to produce solid silver iodide and aqueous lithium nitrate. Aqueous barium chloride and aqueous potas- sium carbonate react to produce solid barium carbonate and aqueous potassium chloride.
Aqueous sodium oxalate and aqueous lead II nitrate react to produce solid lead II oxalate and aqueous sodium nitrate. Describe the result of a double-replacement reaction. Double-replacement reactions produce two different compounds, one being a solid precipitate, water, or gas. Classify What type of reaction is most likely to occur when barium reacts with fluorine? Write the chemical equation for the reaction. A synthesis reaction will likely occur.
Ba F2 0 BaF2 Interpret Data Does the following reaction occur? Section 9. Describe the four types of chemical reactions and their characteristics. Synthesis: two substances react to yield a single product. Combustion: a substance reacts with oxygen, producing heat and light. Decomposition: a single compound breaks down into two or more elements or new compounds. Replacement: the atoms of one element replace the atoms of another element in a compound singlereplacement , or positive ions are exchanged between two compounds double-replacement.
Use NR to indicate if no reaction occurs. Lil aq In a single-replacement reaction, atoms of one element replace atoms of another element in a compound. In a double-replacement reaction, two compounds dissolved in water exchange positive ions. Aqueous solutions of potassium iodide and silver nitrate are mixed, forming the precipitate silver iodide.
Aqueous solutions of ammonium phosphate and sodium sulfate are mixed. No precipitate forms and no gas is produced. Aqueous solutions of lithium sulfate and calcium nitrate are mixed, forming the precipitate calcium sulfate. Challenge When aqueous solutions of sodium carbonate and manganese V chloride are mixed, a precipitate forms. The precipitate is a compound containing manganese. Mixing sulfuric acid H2SO4 and aqueous potassium hydroxide produces water and aqueous potassium sulfate.
Mixing hydrochloric acid HCl and aqueous calcium hydroxide produces water and aqueous calcium chloride. Mixing nitric acid HNO3 and aqueous ammo- nium hydroxide produces water and aqueous ammonium nitrate.
Mixing hydrosulfuric acid H2S and aqueous Hydrobromic acid HBr reacts with aqueous calcium hydroxide produces water and aqueous calcium sulfate.
Perchloric acid HClO4 reacts with aqueous Nitric acid HNO3 reacts with aqueous potassium rubidium sulfide, forming hydrogen sulfide gas. Challenge Aqueous potassium iodide reacts potassium carbonate, forming carbon dioxide gas and water. Sulfuric acid H2SO4 reacts with aqueous sodium cyanide, forming hydrogen cyanide gas and aqueous sodium sulfate.
List three common types of products produced by reactions that occur in aqueous solutions. Describe solvents and solutes in an aqueous solution. A solvent is the most plentiful substance in a solution, and a solute is the substance dissolved in the solvent.
Distinguish between a complete ionic equa- tion and a net ionic equation. A net ionic equation includes only the particles that take part in the reaction.
Write complete ionic and net ionic equations for the reaction between sulfuric acid H2SO4 and calcium carbonate CaCO3. Analyze Complete and balance the following equation. Chapter 9 Assessment following reaction be most likely to produce?
Explain your reasoning. The barium and chloride ions are spectator ions; so the ions that take part in the reaction are the OH and H ions, which form water. Formulate Equations A reaction occurs when nitric acid HNO3 is mixed with an aqueous solution of potassium hydrogen carbonate. Aqueous potassium nitrate is produced. Write the chemical and net ionic equations for the reaction. Define chemical equation.
A chemical equation is a representation of a chemical reaction using chemical symbols, arrows, and numbers to indicate the reactants and products. Distinguish between a chemical reaction and a chemical equation. A chemical reaction occurs when reactants are converted into products. A chemical equation is a representation of a chemical reaction using chemical symbols. The chemical equation also indicates the physical state of the reactants and products.
Explain the difference between reactants and products. Reactants are the initial components and products are the resultant components. What do the arrows and coefficients in equa- tions communicate? Arrows separate reactants from products and specify direction of reaction. Coefficients specify the relative amount of the components. Does a conversion of a substance into a new substance always indicate that a chemical reaction has occurred? A chemical reaction is the process by which the atoms of one or more substances are rearranged to form different substances.
Write formulas for the following substances and designate their physical states. Identify the reactants in the following reaction: When potassium is dropped into aqueous zinc nitrate, zinc and aqueous potassium nitrate form. Balance the reaction of hydrogen sulfide with atmospheric oxygen gas. Write word equations for the following skeleton equations. Balance the following reactions. Hydrogen iodide gas breaks down into hydrogen gas and iodine gas during a decomposition reaction.
Write a skeleton equation for this reaction. Write skeleton equations for these reactions. Write a skeleton equation for the reaction between lithium s and chlorine gas to produce lithium chloride s. Write chemical equations for these reactions.
When solid naphthalene C10H8 burns in air, the products are gaseous carbon dioxide and liquid water. Bubbling hydrogen sulfide gas through manganese II chloride dissolved in water results in the formation of the precipitate manganese II sulfide and hydrochloric acid. Solid magnesium reacts with nitrogen gas to produce solid magnesium nitride.
Heating oxygen difluoride gas yields oxygen gas and fluorine gas. Balance the skeleton equations for the reactions described in Question List each of the four types of chemical reactions and give an example for each type. How would you classify a chemical reaction a.
Under what conditions does a precipitate form in a chemical reaction? Will a metal always replace another metal in a compound dissolved in water? The most active metal will replace the least active metal, but the opposite will not occur.
In each of the following pairs, which element will replace the other in a reaction? Classify this reaction. Write a balanced chemical equation for the combustion of liquid methanol CH3OH. Write chemical equations for each of the following synthesis reactions. Classify each of the reactions represented by the chemical equations in Question Use Figure 9.
Combustion Write a chemical equation for the combustion of each of the following substances. If a compound contains carbon and hydrogen, assume that carbon dioxide gas and liquid water are produced. Write chemical equations for each of the a. Write a chemical equation for the reaction between the two compounds shown in the figure. One or more products may be identified. Write chemical equations for the following single-replacement reactions that may occur in water.
If no reaction occurs, write NR in place of the products. Complete the following word equation.
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