Chemistry

Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 4Al (s) + 3O2 (g) →→ 2Al2O3 (s) The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is ________ g.
Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide:

4Al (s) + 3O2 (g) 2Al2O3 (s)

The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is ________ g.

A)5.3
B)7.4
C)4.7
D)9.4
E)5.0

  1. 👍
  2. 👎
  3. 👁
  1. 4 moles Al to 3 moles O2

    molar masses ... Al - 27 g ... O2 - 32 g

    moles Al ... 2.5 / 27 ... 0.093 ... dividing by 4 = .023
    moles O2 ... 2.5 / 32 ... 0.078 ... dividing by 3 = .026

    Al is the limiting reactant ... 0.069 moles of O2 are consumed ... 3 * .023
    ... 32 g * .069 = ? ... added to 2.5 g of Al

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas. Is Al2(CO3)3 ==> Al2O3 + CO2 the right equation? If so, how do you balance this equation?

  2. chem

    a considerable amount of heat is required for the decomposition of aluminum oxide. 2Al2O3-> 4Al(s)+ 3O2(g) change in heat= 3352KJ a. what is the heat change for the formation of 1 mol of aluminum oxide from its elements? i got

  3. 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

  4. Chemistry

    1. Aluminum reacts with oxygen to produce aluminum oxide which can be used as an adsorbent, desiccant or catalyst for organic reactions. 4Al(s) + 3O2(g) → 2Al2O3(s) A mixture of 82.49 g of aluminum ( Picture = 26.98 g/mol) and

  1. chemistry

    Consider the reaction of solid aluminum iodide and potassium metal to form solid potassium iodide and aluminum metal. The balanced chemical equation is AlI₃(s) + 3 K(s) → 3 KI(s) + Al(s). Given the reaction has a percent yield

  2. chemistry

    can you calculate the mass(g) of AL2O3 that is produced when 2.5g of aluminum and 2.5g of oxygen react according to this equation : 4Al(s)+3O2(g)->2Al2O3(s) im not understanding how to do this

  3. Chemistry

    What is the chemical equation for solid aluminum reacts w/ solid iodine to produce solid aluminum iodide?

  4. Chemistry

    A- 50.0 g of H2SO4 react with 75.0 g of NaOH. Identify the limiting and excess reactants. How many grams of Na2SO4 will be formed? B- A chemist burns 160.0 g of aluminum in 200.0 g of oxygen. She produces 275.0 g of aluminum

  1. Chemistry

    Bauxite ore contains aluminum oxide Al2O3(s) which is decomposed using electricity to produce aluminum metal and oxygen gas. What mass of aluminum metal can be procuced from 155g of aluminum oxide?

  2. 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

  3. Chemistry

    Aluminum reacts with oxygen gas to produce aluminum oxide. How many moles of aluminum oxide would you expect to produce if you reacted 14.5 moles of oxygen gas with excess aluminum? 4Al +3O2 --> 2Al2O3 14.5 mol O2 x 4 mol Al / 3

  4. Chemistry

    In a chemical reaction, 10 moles of the element aluminum react with 7.5 moles of oxygen gas. This produces 5 moles of aluminum oxide (Al2O3). 20Al + 15O2 → 10Al2O3 4Al + 3O2 → 2Al2O3 Al + O2 → Al2O3 10Al + 7.5O2 → 5Al2O3

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