University:
Bradley University
Course:
CHM 100 | Fundamentals of General Chemistry
Academic year:

2023
Views:

89

Pages:

2
Author:

Triston Franco

NSM 12C PAL Worksheet Reactions & Stoichiometry Name: ______________ Part I: Write and balance the following reactions: include all states (s), (l), (g) and (aq). Hints: Most metals are solids under normal conditions. Some elements are gasses under normal conditions. All ionic compounds are solids on their own. Any substance in a solution of water is considered to be aqueous. Nitrogen and hydrogen react to form ammonia gas. ______________________________________________________________________________ Liquid water decomposes into its elements. ______________________________________________________________________________ Methane gas undergoes combustion to form ______ & ______ (you should know the products). ______________________________________________________________________________ Sodium reacts with water to form hydrogen gas and a solution of sodium hydroxide. ______________________________________________________________________________ Solutions of lead (II) nitrate and barium chloride react to form solid lead (II) chloride and a solution of barium nitrate. ______________________________________________________________________________ Solutions of nitric acid and potassium hydroxide react to form water and aqueous potassium nitrate. ______________________________________________________________________________ Solid sodium carbonate is added to a solution of hydrochloric acid. Aqueous sodium chloride, water and carbon dioxide are produced. ______________________________________________________________________________ Part II Stoichiometry: Refer to the balanced equations in Part I. 1. How many grams of sodium are needed to react with 205g of water in the reaction that produced hydrogen gas and aqueous sodium hydroxide? 2. If 5.0g of nitrogen and 5.0g of hydrogen react, how many grams of ammonia will form? A) Which reactant is the limiting reactant? Excess reactant? B) How many grams of the excess reactant remain? (There are two ways to determine)