LWR # 1 Apply Stoichiometry A student performed an experiment to find the amount of sodium carbonate, (Na₂CO₂) that is produced from the decomposition of baking soda, NaHCO, by heating. Decomposition of baking soda: 2NaHCO,> Na₂CO, + CO₂ + H₂O The following data were collected. Complete the data table. Mass of empty evaporating dish 24.353 grams Mass of evaporating dish and baking 27.868 grams soda 26.885 grams Mass of evaporating dish and sodium carbonate Mass of baking soda 84.007 g/mol Mass of sodium carbonate (experimental) 105.9888 g/mol Molar mass of baking soda 84.007 g/mol Molar mass of sodium carbonate 105.9888 g/mol 1.678 grams > 4 Theoretical (calculated) mass of sodium carbonate 09314 g/mol Calculate percent error of the analysis (1105.9888-09314) +100/.09314 = 9.8% 1 = Atomic mass: Na = 23.0g; H=1.0 g; C=12.0g; O=16.0g % error = (Experimental-Calculated) x 100/ Calculated

Consider the reaction of copper(II) oxide with aluminum metal to produce copper metal and aluminum oxide: 3 CuO(s) + 2 AlI(s) → 3 Cu(s) + Al2O3(s) If 7.99x1023 atoms Al react with an excess of CuO, what mass of Cu(s) is produced? Assume the reaction goes to 100% completion. Enter your response in decimal notation to three significant figures. Answer: Enter Value g.

To produce zinc metal, carbon monoxide reacts with zinc (I1) oxide according to: Zno + CO - Zn + CO2 The carbon monoxide, however, is initially prepared from: 2C+ 02 → 200 How many grams of zinc metal (Zn) may be prepared if If 81.0g of C is used with excess amount of ZnO? Your answer should be numerical and neglect units (e.g., if you calculate 3.5g then input 3.5).

The reaction below takes place in water at room tempeture. Balance the reaction and write the correct state of matter for the substance.  CaCI_2(aq) + (NH_4)_3PO_4 -> Ca_3(PO_4)_2 + NH_4CI

Soda ash (sodium carbonate) is widely used in the manufacture of glass.  Prior to the environmental movement much of it was produced by the following reaction.   CaCO3 + 2 NaCl → Na2CO3 + CaCl2   Unfortunately, the byproduct calcium chloride is of little use and was dumped into rivers, creating a pollution problem.  As a result of the environmental movement, all of these plants closed.  Assume that 125g of calcium carbonate (100.09 g/mol) and 125 g of sodium chloride (58.44 g/mol) are allowed to react.   Determine how many grams of useful sodium carbonate (105.99 g/mol) will be produced.  How many grams of useless calcium chloride (110.98 g/mol) will be produced?  You should also determine how many grams of excess reactants are left (indicate which one is the limiting reactant)

Calculate the mass(in grams) of the product formed when 15.40g of  Cl_2(g) completely reacts. Assume that there is more than enough of the other reactant. 2 K(s) + Cl _2(g) --> 2KCl(s)

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3  and water:   2Al(OH)3(s) + Al2O3(s) ->  3H2O(g) In the second step, alumina Al2O3  and carbon react to form aluminum and carbon dioxide:   2Al2O3(s) +  3C(s) + 4Al(s) ->  3CO2(g) Suppose the yield of the first step is 74.%  and the yield of the second step is  76.% . Calculate the mass of aluminum hydroxide required to make  4.0kg  of aluminum.   Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.

Name Lab Partner Section # Date Pre-Lab Assignment: Stoichiometry Lab 1. In a lab experiment similar to the one you are going to do, a student slowly added hy- drochloric acid (HCI) to an evaporating dish containing magnesium carbonate MgCO3. a. Complete and balance the following equation for the reaction between magnesium carbonate and hydrochloric acid. MgCO3 (s) + HCl (aq) → (aq) + H₂CO3(aq) (When writing the formula for the missing product did you consider the charges of the ions?) b. When carbonic acid is formed in a chemical reaction, it is unstable and immedi- ately decomposes into carbon dioxide and water. Rewrite the equation above to show the final products using this information.

Remaining Time! 02:29:4. Consider the balanced chemical equations shown below. When a 6.00 g sample of a mixture of iron (Fe) and aluminum (Al) is treated with excess HCl(aq), 0.177 moles of H2 are obtained. What is the mass percentage of Fe in the original mixture? Choose the closest answer. Fe(s) + 2 HCI(aq) FeCl2(aq) - + H2(g) 2 Al(s) +6 HC((aq) 2 AICI3(aq) + 3 H2(g) 96 % 69 % 47 % 33 % 17 % Rack Question Menu - O O

+ BIUA Normal text Arial 12 二 三1|-山- 1 1 3. 5. If 10.0 gram of aluminum chloride are decomposed, how many molecules of Cl, are produced? | AICI, → Al + Cl2