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!)

  1. 👍 0
  2. 👎 0
  3. 👁 557
  1. 100 (4.78/6.67)

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. 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

    asked by K on October 16, 2007
  2. 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

    asked by Tim H on September 15, 2014
  3. 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?

    asked by Jack on March 1, 2010
  4. 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
  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

    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.

    asked by COR on February 22, 2020
  2. CHEMISTRY

    A student combusted 0.500g of purified aluminum power with excess oxygen in an oxygen atmosphere according to the reaction, 4Al(s) + 3O2(g)= 2Al2O3(s) A) What is the limiting reactant? B) How many moles of Al were used? C) How

    asked by Gina on October 29, 2014
  3. Chemistry

    Write skeleton equations for these reactions. a. hydrogen iodide(g) --> hydrogen(g) + iodine(g) b. aluminum(s)+iodine(s)--> aluminum iodide(s) c. iron(II) oxide(s) + oxygen(g) --> iron(III) oxide(s)

    asked by Lily on November 16, 2010
  4. chem

    A 2.241 g sample of nickel reacts with oxygen to form 2.852 g of the metal oxide. Calculate the empirical formula of the oxide. Give the number of moles of each element to support you answer.

    asked by sam on November 14, 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.