Chemistry, asked by teremererojo, 10 months ago

NaOH +HCl → NaCl+H20 a)How many moles of NaOH is needed to completely react with 1 mole of HCl? b)How many grams of HCl is required to completely neutralise 160g NaOH?

Answers

Answered by Anonymous

Answer:

Chapter 5: Chemical Reactions

CHAPTER OUTLINE

5.1 Chemical Equations

5.2 Types of Reactions

5.3 Redox Reactions

5.4 Decomposition Reactions

5.5 Combination Reactions

5.6 Replacement Reactions

5.7 Ionic Equations

5.8 Energy and Reactions

5.9 The Mole and Chemical

Equations

5.10 The Limiting Reactant

5.11 Reaction Yields

LEARNING OBJECTIVES/ASSESSMENT

When you have completed your study of this chapter, you should be able to:

1. Identify the reactants and products in written reaction equations, and balance the equations by

inspection. (Section 5.1; Exercises 5.2 and 5.6)

2. Assign oxidation numbers to elements in chemical formulas, and identify the oxidizing and reducing

agents in redox reactions. (Section 5.3; Exercises 5.10 and 5.15)

3. Classify reactions into the categories of redox or nonredox, then into the categories of decomposition,

combination, single replacement, or double replacement. (Sections 5.4, 5.5, and 5.6; Exercise 5.20)

4. Write molecular equations in total ionic and net ionic forms. (Section 5.7; Exercise 5.30 a, b, & c)

5. Classify reactions as exothermic or endothermic. (Section 5.8; Exercise 5.34)

6. Use the mole concept to do calculations based on chemical reaction equations. (Section 5.9; Exercise

5.42)

7. Use the mole concept to do calculations based on the limiting‐reactant principle. (Section 5.10;

Exercise 5.52)

8. Use the mole concept to do percentage‐yield calculations. (Section 5.11; Exercise 5.56)

LECTURE HINTS AND SUGGESTIONS

1. Do not get bogged down explaining and defining oxidation numbers. Oxidation numbers can easily

be overemphasized. Their main roles are in recognizing redox reactions and in balancing redox

equations. Focus on those roles as the purpose for learning the rules of oxidation numbers. Make

certain that students understand that oxidation numbers are not charges.

2. Use some simple redox reactions and relate the oxidation number change with the loss and gain of

electrons. For example, in the reaction, 2Na + Cl2 → 2NaCl, each sodium atom loses one electron and

its oxidation number goes from 0 to + 1; and each chlorine atom gains an electron and its oxidation

number goes from 0 to ‐1.

3. Sometimes a concrete example of a limiting reactant helps the student to visualize that concept. One

Explanation:

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