CHE 145 - Lab 10 Single Replacement Reactions Fall 2019 Chemical equations represent chemical changes Creactions that ac

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Che 145 Lab 10 Single Replacement Reactions Fall 2019 Chemical Equations Represent Chemical Changes Creactions That Ac 1 (52.21 KiB) Viewed 66 times

Che 145 Lab 10 Single Replacement Reactions Fall 2019 Chemical Equations Represent Chemical Changes Creactions That Ac 2 (52.99 KiB) Viewed 66 times

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Che 145 Lab 10 Single Replacement Reactions Fall 2019 Chemical Equations Represent Chemical Changes Creactions That Ac 3 (58.26 KiB) Viewed 66 times

Che 145 Lab 10 Single Replacement Reactions Fall 2019 Chemical Equations Represent Chemical Changes Creactions That Ac 4 (39.75 KiB) Viewed 66 times

CHE 145 - Lab 10 Single Replacement Reactions Fall 2019 Chemical equations represent chemical changes Creactions that actually occur. A chemical equation consists of А two parts: 1) the reactants (starting materials), and 2) products. Reactant A+ Reactante Product A+ Product Betc... The major problem in writing a chemical equation is predicting what products will be produced in the reaction. To determine what reactions will take place, we carry out experiments. Using the experimental data obtained from the experiments, we can sometimes predict what products will be formed in a similar type of reaction. There are numerous types of chemical reactions, but we will only perform experiments with single and double replacement reactions, Some Types of reactions are: combination (A + BC) decomposition (C+ A+B) combustion (C.H. + O, CO + H2O) single replacement (ABX BAX) double replacement (ZA-X BAZX() SINGLE REPLACEMENT REACTIONS Two important terms for this experimentare didation and reduction Oxidation occurs when an element loses electrons. Reduction occurs when an element gains electron Oxidation cannot occur without reduction, so reactions where both processes occur are called oxidation-reduction (or redox) reactions, In a single replacement reaction, one element reacts with a compound to produce a new compound, and displaces an element in the original compound. ABX BAX If A is a metal, it will replace the element B (usually another metal or hydrogen) in the compound Bx to form a new compound AX. The element B is now a free metal (or hydrogen gas). Free metals have an oxidation state of zero. The reaction will occur if A is more active than the element B. A metal is said to be more active than another metal if it loses electrons more easily fie is more easily ridized) than the other metal. A ranking of metals based on their relative reactivity and ease of oxidation is called an activity series. By knowing which elements are at the top of the list, we can predict whether or not a reaction will occur. The elements on the top of the list will replace any element underneath it on the list. K Most active Potassium is most easily oxidised: K+K+ Ca AI Fe Sn Hg Pt
CHE 145 - Lab 10 Single Replacement Reactions Fall 2019 For example, if a solid piece of Ca metal was placed in a solution of tin(ll) nitrate, the Ca would dissolve and the tin metal would come out of solution, Calcium est electrons den - Ca(s) + Sn(s) + Ca(NO(a) Sn(NO)2 (aq) Tinca_electrons relart pt must be high + This is a typical single replacement reaction. Calcium is more active (more easily oxidized) than tin. Another way to think about it is that tin removes the electrons from calcium (.e. tin is reduced). If the free metal is lower on the list (less reactive) than the metal attached to the anion, no reaction would occur (NR) Pt FeCl- NR In this experiment, various metals will be placed into solutions of metal ions or into a solution of hydrochloric acid. The reactions will be observed and noted. An activity series will be constructed ranking the elements according to which elements reacted with the most solutions of metal ions. Materials: 0.1 M solutions of the following: Cu(NO). Zn(NO), Me(NO)Fe(NO J. and Pb(NO3)2 6 M HCl and 9 MH.SO. Four 4x3 well plates Procedure: 1. Obtain five pieces each of the metals copper, zinc, iron and lead. Obtain one long piece of Mg ribbon 2. Polish the magnesium ribbon with a piece of emory cloth or sandpaper, and cut into five pieces. 3. Place a piece of copper in each of the 5 wells in the first vertical column of your well plate as indicated by the table. 4. Repeat step 3 with the Zn, Mg, Fe, and Pb. 5. Add 8 drops of 6 M HCl to each metal in the first row. For the lead (Pb), use 9 MH.SO. Instead of 6 M HCI 6. Record you observations in the table below. Look for bubbles or changes to the metal surface. Some reactions may require five minutes or so for a noticeable change to occur. 7. Add 8 drops of 0.1M solutions of Cu(NO). Zn(NO), Mg(NO3), Fe(NO) and Pb(NO) to each row of metals as indicated on the table. 8. After recording your observations, discard the solutions (and metal pieces) in the proper container in the hood, rinse the well plates with distilled water and dry with a paper towel. CAUTION!! 6 M HCl and 9 MH,SO, can burn your skin. If you get some on your skin, flush with water immediately for a minimum of 15 minutes. Inform your instructor of any chemical contact as soon as possible CAUTION!! Lead is harmful if injested. Wash your hands after this portion of the lab
Observations: Use "NR" if no reaction appeared to occur. Cu Zn Mg Fe Pb HCI USE OM HISO NR Bay Bubbling tunt bubbles Cu(NO) change color change alo slow rete change color Zn(NO3)2 NR. 2 bung NA Mg(NO3)2 NR NA Fe(NO3) NR Jos oligoft tretants Pb(NO3)2 va Colont Bullig dissolving solo and NR IR WR Cu + HCI Using the above information write a balanced equation for each reaction which occurred. If no reaction occurred, write "NR". Be sure to show the proper phases (.e.g. solid (s) or aqueous (aq)). More active Less active (5), (a), (g) Element Element H₂ HCI ZnCl2 (1) + H₂O Zn H₂ Mg)* HCI Fe HCI NR Zn(s)+ + Pb(+ HSO4 Zn) + Cu(NO) CA Mg(s) + Cu(NO3)2 Cu(NO3)2 Znale Et Ca (5) Zn Fe + Po + Cu(NO) Culo) Zn(NO:), NR Mg)" + Zn(NO) Fe + Zn(NO3)2 NRT Pb + Zn(NO) Cu 67 Mg(NO3)2 NB (5) 3
Fall 2019 CHE 145 - Lab 10 Single Replacement Reactions Zn + Mg(NO3): Fe + Mg(NO3)2 Mg(NO3)2 Pb + Cu + Fe(NO) Zn + Fe(NO) Fe(NO) Mg Pb + Fe(NO) Cu Pb(NO) Zn + Pb(NO3)2 Mg + Pb(NO3)2 Fe + Pb(NO3)2 Based on the above information, assign an activity order to each of the metals (most active = 1) 1 2 3 4 1. Sometimes magnesium metal is used to protect steel-hulled ocean going vessels from corrosion. Suggest a way in which this protection might work. 2. Based on your activity series, explain why the Statue of Liberty was made with copper instead of zinc. 3. Based on your experimental data of relative chemical activity among these metals: a. Which metal is most likely to be found in the uncombined or "free" state in nature? Explain b. Which metal would be least likely to be found uncombined with other elements? Explain c. Which are more easily oxidized, metals or non-metals? Explain.