How many grams of Cl, are needed to form 79.3 g of AlCl₂? 2 Al(s) + 3 Cl₂(g) → 2 AICI, (s) Step 1: Show the strategy for solving this problem. grams AICI, Answer Bank grams Cl, moles Cl₂ moles Al moles AICI, grams Al grams AICI, Step 2: Show the conversions required to solve this problem and calculate the grams of Cl.. 79.3 g AICI, X =g Cl₂ Answer Bank 70.90 g C₂ grams of Cl₂: 26.98 g Al 1 mole Cl 1 mole Al 1 mole AICI, 2 moles Al 3 moles Cl₂ 133.33 g AICI, 2 moles AICI, grams Cl₂ g Cl₂

How many grams of Cl, are needed to form 79.3 g of AlCl₂? 2 Al(s) + 3 Cl₂(g) → 2 AICI, (s) Step 1: Show the strategy for solving this problem. grams AICI, Answer Bank grams Cl, moles Cl₂ moles Al moles AICI, grams Al grams AICI, Step 2: Show the conversions required to solve this problem and calculate the grams of Cl.. 79.3 g AICI, X =g Cl₂ Answer Bank 70.90 g C₂ grams of Cl₂: 26.98 g Al 1 mole Cl 1 mole Al 1 mole AICI, 2 moles Al 3 moles Cl₂ 133.33 g AICI, 2 moles AICI, grams Cl₂ g Cl₂

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 150AE: You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of...

See similar textbooks

Similar questions

A Menthol, from oil of mint, has a characteristic odor. The compound contains only C, H, and O. If 95.6 mg of menthol burns completely in O2, and gives 269 mg of CO2 and 111 mg of H2O, what is the empirical formula of menthol?
3.81 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients.
You have seven closed containers, each with equal masses of chlorine gas (Cl2) . You add 10.0 g of sodium to the first sample, 20.0 g of sodium to the second sample, and so on (adding 70.0 g of sodium to the seventh sample). Sodium and chlorine react to form sodium chloride according to the equation 2Na(s)+Cl22NaCl(s) After each reaction is complete, you collect and measure the amount of sodium chloride formed. A graph of your results is shown below. Answer the following questions: a. Explain the shape of the graph. b. Calculate the mass of NaCl formed when 20.0 g of sodium is used. c. Calculate the mass of Cl2 in each container. d. Calculate the mass of NaCl formed when 50.0 g of sodium is used. e. Identify the leftover reactant, and determine its mass for parts b and d above.
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reac- tion has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. D Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
Please fill in the rest of the table to figure out the theoretical yield of the biodiesel. Some other things to know is that the molar ratio of vegetable oil to methanol is 1:6 but in the picture, you can see that it says 3 equivalence of methanol. I was a bit confused on this, but hopefully it helps. Compound MW (g/mol) V (mL) d (g/mL) Weight (g) Mols Equivalence Vegetable oil 882 g/mol 12 mL 0.91-0.92 g/mL Methanol 32 g/mol 3 mL 0.791 g/mL Biodiesel 250-290 g/mol N/A 1.26 g/mL
A student mixes magnesium and hydrochloric acid and a chemical reaction occurs, shown in the equation below. ____ Mg + _____ HCl --------> _____ H2 + ______ MgCl a. Balance the chemical equation, then label the reactants and the products. b. What do the coefficients in the chemical equation represent? c. What does it mean if an element or molecule does not have a coefficient? d. How many moles of magnesium would you need for the reaction if you had 2 moles of HCl? e. How many moles of magnesium would you need for the reaction if you had 4 moles of HCl? f. How many moles of hydrogen gas (H2) would be produced if you started with 2 moles of magnesium and 2 moles of hydrochloric acid (HCl)? g. If you started with 2 moles of magnesium and 6 moles of hydrochloric acid (HCl), which one would be your limiting reactant? Which one would be your excess reactant? h. Using the information from part e, how many moles of…
Your lab partner accidentally mixed some sodium chloride with your sample of Epsom salts (MgSO₄･7H₂O). You want to make a standard solution of magnesium ion, and this is the only sample of a magnesium salt you have. To determine the amount of magnesium salt in the mixture, you heat 100.00 g to drive off the water of hydration and find that the anhydrous mixture has a mass of 57.75 g. How many grams of the original salt mixture must you add to 1.000 L of water to make a 0.100 M solution of Mg²⁺ ion?
DEET, C12H17NO, is the active ingredient in many insect repellents. If you want to produce 25.0 mg of DEET from the reaction of C8H7OCl and C4H11N, what is the minimum amount of C4H11N that is needed? C8H7OCl (l) + C4H11N (l) -> C12H17NO (l) + HCl (g) MULTIPLE CHOICE: A) 2.50 x 101 g B) 9.56 x 100 g C) 9.56 x 10-3 g D) 3.50 x 102 g E) 4.04 x 10-2 g
calculate the masses of both reactants and products assuming a 100% reaction. Na3PO3 + CaCl2 = Ca3(PO3)2 NaCl 3.2g 2.6g