se the following information to answer this question. CAle) + 3CuClz(ag)→2AICI3(aq) + 3Cu(s) word equation: aluminum plus three copper(II) chloride produce two aluminum chloride and three copper) Which of the following best describes what is occurring during this reaction? Select one: O a. Aluminum replaces chlorine in the compound. O b. Aluminum replaces copper in the compound. O c. Copper replaces aluminum in the compound. O d. Chlorine replaces copper in the compound. Smoke Signal.pdf

write balanced equation for the following questions. 1. A reaction occurs that produces iron(III) sulfide from its elements. 2. Oxygen gas and sodium chloride are produced from the decomposition of sodium hypochlorite. 3.Nitrogen gas is combusted to produce nitrogen dioxide gas. 4. Aluminium bromide solution reacts with chlorine gas. 5. Aluminium iodide solution reacts with thallium(I) nitrate solution.

Specify which of the following are oxidation-reduction reactions, and if it is, identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. If it is not, select No and leave the following boxes blank. Express your answers as chemical formulas. Omit states-of- matter. a. b. CH4 (9) + 302(g) → CO2 (g) + 2H₂O(g) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced 3AgNO3(aq) + Sc(s) → Sc(NO3)3(aq) + 3Ag(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced î

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Balance Equation: 2Al + 3CuCl2 * 2H2O -> 2Cu + 2AlCl3 + 6H20 1. Reproduce the following table in your document. Write the chemical reaction again in the indicated spot, typing the reactants under the word “reactants” and products under the word “products”. Then in the row labeled “Element”, list each element in the reactants and products. Assign oxidation numbers to each element in the reactants and products and write the oxidation number underneath each element in the table below. Explain how these were derived. (see table) 2. From the reactants, identify the oxidizing agent and reducing agent and input this into the table above. Explain, in a few sentences, how you determined the difference between the two. 3. Type out the complete ionic equation and the net ionic equation for the reaction. Explain how you arrived at your answer in a narrative (3-5 sentences), including why you canceled any ions as spectators.

For each of the following sets of reactants, write the balanced equation for the single displacement reaction that occurs. If you determine that a reaction will not occur, write “NR”, and provide a brief explanation.  a. Aluminum metal + aqueous nickel(II) nitrate b. Gold metal + hydrobromic acid

Balance this chemical equation. Include the states of matter.   A solid of aluminum sulfate reacts with a solution of barium chloride yielding a solution of aluminum chloride and a solid of barium sulfate.

Great work! 3. Pick a "for every" statement about copper and silver in this balanced reaction. 29 47 Cu Ag Copper 63.55 Silver 107.87 Hint: The correct balanced equation is Cu + 2A9NO, → 2Ag + Cu(NO,)2 For every 1 mole of copper, the reaction makes 2 moles of silver. For every 1 mole of copper, the reaction uses up 2 moles of silver. For every 1 mole of copper, the reaction makes 1 mole of silver. Submit Answer 3/3 submissions remaining Score:

For each question, do the following four things: 1. Predict the products that will be made in this double replacement reaction. 2. Write the formulas for each substance. 3. Record the states of matter. 4. Balance the equation.

FIRST, write the balanced equation that represents each reaction. THEN, classify each reaction. a) Hydrochloric acid neutralizes barium hydroxide b) Propane (C3H8) is burned. c) Chromium and oxygen form chromium (III) oxide. (Skip classifying this reaction; we will learn this reaction next week) d) Ammonium carbonate and barium chloride are mixed; barium carbonate precipitates.