CHEM-last part prob.

Aluminum reacts with chlorine gas to form aluminum chloride via the following reaction:

2Al(s) + 3Cl2(g) -> 2AlCl3(s)

You are given 19.0g of aluminum and 24.0g of chlorine gas.

a)If you had excess chlorine, how many moles of of aluminum chloride could be produced from 19.0g of aluminum?
= 0.704mol AlCl3

b)If you had excess aluminum, how many moles of aluminum chloride could be produced from 24.0g of chlorine gas, Cl2?
=0.255mol AlCl3

By comparing your answers for Parts A and B, you can determine which reactant is limiting. Keep in mind that the limiting reactant is the one that produces the lesser amount of product.

what exactly do I do to solve for part "c"?????

c)What is the maximum mass of aluminum chloride that can be formed when reacting 19.0g of aluminum with 24.0g of chlorine?
answer:_____g AlCl3

is it?: 0.704mol AlCl3-0.255molAlCl3=0.449mol AlCl3 x 226.6g/mol = 119.7g AlCl3?

  1. 👍 0
  2. 👎 2
  3. 👁 3,898
  1. I tried this answer & it was incorrect.

    1. 👍 0
    2. 👎 0
  2. First, I don't get 0.255 for mols AlCl3 formed from 24.0 g Cl2.
    I get 24/71 x (2 mols AlCl3/3 mols Cl2) = 0.338 x 2/3 = 0.225 mols AlCl3.
    Check my arithmetic.

    Then the answer to part c is simple. Notice that the problem says, and I quote, "Keep in mind that the limiting reactant is the one that produces the lesser amount of product." So which produces the lesser amount of product? Of course that is the 24 g Cl2 so 0.225 mols AlCl3 (which is smaller than 0.704) is the # mols and that times the molar mass AlCl3 will give you the mass AlCl3. I get 0.225 x 133.3 = 30.03 g which is rounded to 30.0 to three significant figures. Check my work closely. I think 30.0 is the answer to part c but you try it, too.

    1. 👍 1
    2. 👎 0
  3. ok...so I shouldn't have multiplied through by 2. That makes a lot more sense. Thank you, yet again, and it came out alright.

    1. 👍 0
    2. 👎 0
  4. (oh...slightly dislexic...yes...I meant 0.225 moles, that would have helped if I had noticed before & typed it in correctly.)

    1. 👍 0
    2. 👎 0
  5. Chemlast champer vacancies

    1. 👍 0
    2. 👎 0
  6. how do you do part a?

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    What is the maximum mass of aluminum chloride that can be formed when reacting 30.0 g of aluminum with 35.0 g of chlorine?

    asked by Summer on September 21, 2008
  2. Chemistry

    Nitrogen reacts with powdered aluminum according to the reaction: 2Al(s)+N2(g)→2AlN(s) How many liters of N2 gas, measured at 892 torr and 98 ∘C, are required to completely react with 17.8 g of Al?

    asked by Leslie on May 4, 2018
  3. Chemistry

    The balanced equation for the reaction of aluminum metal and chlorine gas is 2Al(s) + 3Cl2(g) → 2AlCl3(s) Assume that 0.40 g Al is mixed with 0.25 g Cl2. What is the maximum amount of AlCl3, in grams, that can be produced?

    asked by John on June 11, 2020
  4. Chemistry

    Aluminum sulfate reacts with calcium hydroxide (from lime) to form aluminum hydroxide and calcium sulfate. Write the balanced formula unit equation for the reaction.

    asked by Ana on September 28, 2014
  5. chemistry

    when aluminum metal reacts with iron (III) oxide to form aluminum oxide and iron metal, 429.6 kJ of heat are given off for each mole of aluminum metal consumed, under constant pressure and standard conditions. What is the correct

    asked by sylvia on December 2, 2008
  1. Chemistry

    In a reaction chamber, 3.0mol of aluminum is mixed with 5.3mol Cl2 and reacts. The reaction is described by the following balanced chemical equation. 2Al + 3Cl2 ==> 2AlCl3 a)Identify the limiting reagent for the reaction.

    asked by Jack on April 5, 2010
  2. Chemistry 1300

    1) Aluminum metal reacts with chlorine gas to form solid aluminum trichloride, AlCl3. What mass of chlorine gas (Cl2) is needed to react completely with 163 g of aluminum? 2) Magnesium (used in the manufacture of light alloys)

    asked by William T on September 12, 2014
  3. chemistry

    A 4.78-g sample of aluminum completely reacts with oxygen to form 6.67 g of aluminum oxide Use this data to calculate the mass percent composition of aluminum in aluminum oxide. (Sorry need help with this!)

    asked by Luis on September 27, 2014
  4. Chemistry

    Write and balance equations for the following reactions. A)Iron metal and Chlorine gas react to form solid iron(III) chloride. B)Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. C)Solid

    asked by Jack on February 28, 2010
  5. Chemistry

    Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Al. Find the theoretical yield (in grams) of manganese from the reaction

    asked by Liz on October 8, 2009

You can view more similar questions or ask a new question.