2Al + Fe2O3 ( Al2O3 + 2Fe (26.98) ( 159.7) (101.96) 124 601 80 b. Al c. 234.3 d. 234 e. 34.1% 1c. A strip of zinc metal with a mass of 2.0g undergoes single displacement reaction with an aqueous solution containing 2.5g of silver(I) nitrate A. Write a balance equation for the above reaction B. Which of the 2 reactants is the limiting reagent? C. Calculate the mass of zinc (II) nitrate formed D. How much excess reagent is left at the end of the reaction?
First, we had to calculate how many grams of copper (II) sulfate we needed to form 100 mL of a 0.200 M solution of copper (II) sulfate. We determined that we needed to use 4.994g of copper (II) sulfate to make the solution. We added distilled water to the 4.994g of copper (II) sulfate in a beaker until it reached 100 mL. Then we put the beaker on a hot plate and added a magnetic stirrer. We determined that the mass of zinc necessary to completely react with the copper (II) ions in the solution was 1.308g.
When referring to mass sum of the atomic masses of the atoms represented by the formula of a molecular substance, the correct term used is A. atomic mass B. formula weight C. molecular mass D. molecular weight 12. A mole of CO2 contians A. 6.02 x 1023 ions C. 6.02 x 1023 formula ions B. 6.02 x 1023 molecules D. 6.02 x 1023 atoms 13. The mass of the products in a chemical reaction depends on the amount of A. excess reactant B. limiting reactant C. oxidizing agent D. reducing subtannce 14.
So, qwater = qmetal Using the formula qmetal = m × c × ΔT, calculate the specific heat of the metal. Use the data from your experiment for the metal in your calculation. Part II: Calculate the energy change (q) of the surroundings (water) using the enthalpy equation qwater = m × c × ΔT. We can assume that the specific heat capacity of water is 4.18 J / (g × °C) and the density of water is 1.00 g/mL. Show ALL your work.
Create reactions with anion placeholders for copper compound and Zinc. If the copper is cuprous, or Cu+1, the reaction is: 2Cu+1(A-1) (aq)+ Zn+2(s) Zn+2(A-1)2 (aq)+ 2Cu+1(s) (A= anion) If the copper is cupric, or Cu+2, the reaction is: Cu+2(A-1)2 (aq) + Zn+2(s) Zn+2(A-1)2 (aq) + Cu+2(s) Calculate the grams of Zinc needed for the reaction if copper compound is cuprous (+1) or cupric (+2). If the Copper is Cuprous: 2Cu+1(A-1) (aq) + Zn+2 (s) Zn+2(A-1)2 (aq) + 2Cu+1(s) Grams of Zn = 1 gram of Cu(A) The amount of Cu(A) that will be used. 1 mol of Cu(A) Divided by the molar mass of Cu(A) 170.49 grams of Cu(A) as given by the instructor. 1 mol of Zn Multiplied by the mole ratio of Zn to Cu(A) 2 mol of Cu(A) in the reaction.
The mass of the oxygen is resulted from the difference between the masses of product oxide and limiting reagent. In equation 1, the mass of limiting reagent magnesium is found. The mass of the oxide product is determined using equation 2. In equation 3, the amount of oxygen in magnesium oxide is found using the weights of the results found in equation 1 and 2. The mass of the oxygen in the oxide product will represent how much added weight was gained in the reaction.
Gas Volume Determination Lab Objective: Use stoichiometry and ideal gas law to predict gas production. Successfully collect gas being produced. Introduction: Write an introduction. Materials: Small flask 100 mL graduated cylinder 5 mL graduated cylinder Rubber stopper Tubing Tubing/Stopper connector Water basin 6M HCl Zinc metal Ring Stand if needed Clamp if needed Copper wire Metal cutters Procedure: 1. Obtain between 0.1 to 0.2g of zinc metal.
Year 11 Chemistry Electrochemical Cells Purpose To determine the order of reactivity for the metals copper, iron, lead and zinc using the least amount of electrochemical cells as possible. Materials List • Four 100ml beakers • 4 strips of filter paper approximately 15cm in length • Voltmeter • Sodium Chloride solution at 10% concentration • Zinc, Copper, Lead and Iron metal strips (approximately 10 cm) • 50 ml of Copper sulphate, Zinc sulphate, Lead nitrate and Iron nitrate solutions • Scissors Procedure - Place the 50ml solution of zinc sulphate in a 100ml beaker, and 50ml solution of copper sulphate in a different 100ml beaker. Place the zinc metal strip in the zinc sulphate beaker and the copper metal strip with the copper sulphate beaker.
Centigram balance: Weighing by difference a) Obtain the second centigram balance. b) Obtain 100ml beaker, and record the mass. c) Transfer the copper slug from the first part of the experiment to the beaker. d) Weigh and record the mass of the beaker + slug. e) Determine the mass of the slug by subtracting the mass of the beaker alone from the mass of the beaker + slug.
Who is right, John or Anna? Explain your answer. 3 When 200 g of calcium nitrate, Ca(NO3)2.2H2O is heated at 120ºC the mass decreases by 36 g. (a) Why does the mass decrease? (b) How much calcium nitrate is left after heating? 4 Calculate the molar mass of these compounds: (relative atomic masses: H = 1; N = 14; O = 16; S = 32; Cu = 64; Br = 80; Pb = 207) (a) copper nitrate, Ca(NO3)2 (b) lead bromate, Pb(BrO3)2 (c) ammonium sulfate, (NH4)2SO4 5 The equation for the complete combustion of methane is shown below.