Chemistry

Al(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2(g)

What is the coefficient of H2 in the balanced equation, obtained by using oxidation numbers?

  1. 👍
  2. 👎
  3. 👁
  1. 2Al(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2(g)
    ..0x2 = 0..2*1+ = 2.........2*3+ = 6..............0
    multiply Al half by 1 and multiply H2SO4/H2 half by 3 to give

    2Al(s) + 3H2SO4(aq) → Al2(SO4)3(aq) + 3H2(g)

    1. 👍
    2. 👎
    👤
    DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    What is the minimum amount of 6.0 M H2SO4 necessary to produce 19.0 g of H2(g) according to the reaction? 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)

  2. Chemistry

    Alumminum hydroxide reacts with sulfuric acid as follows: 2Al(OH)3+H2SO4-->Al2(SO4)+6H2O. Which reagent is the limiting reactant when 0.500 mol Al(OH)3 and 0.500 mol H2SO4 are allowed to react? How many moles of Al2(SO4)3 can form

  3. Chemistry

    Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 14.5g . 1.) What minimum mass of H2SO4 would you

  4. science (chem)

    consider the fo9rmula for Al2(SO4)3,which is used in perspirants: a. how many moles of sulfur are present i 3.0 moles of Al2(SO4)3 b. ow many moles of aluminum ions are present in 0.40 mole of Al2(SO4)3 for a and b i multiplied by

  1. SCIENCE/CHEM

    when the following equation is balanced , what is the sum of the co-efficients? AL2(SO4)^3+Ca(OH)2-->Al(OH)3+CaSO4

  2. Chemistry

    According to the reaction 2Al+3H2SO4→3H2+Al2(SO4)3, the total number of moles of H2SO4 needed to react completely with 5.0 mol of AL is 1. 2.5 mol 2. 5.0 mol 3. 7.5 mol 4. 9.0 mol

  3. Chemistry

    What would be the steps to solving this problem? The aluminum sulfate hydrate [Al2(SO4)3 (times) xH2O] contains 8.20 % Al by mass. Calculate x, that is , the number of water molecules associated with each Al2(SO4)3 unit.

  4. chemistry

    In a solution of Al2(SO4)3 the Al3+ concentration is .12 M. What mass of Al2(SO4)3 is in 50 mL of this solution. Please explain the steps. Thanks. The Al3+ part confuses me the most.

  1. chem

    Sulfuric acid can dissolve aluminum metal according to the following reaction. 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 26.8 g . 1.What minimum amount of H2SO4 in

  2. chemistry urgent

    given the reaction: 2 Al + 3 H2SO4 -> Al2(SO4)3 + 3 H2 what volume of H2 gas measured at STP will be produced from 5.4 grams of AL reacting with an excess of H2SO4?

  3. Chemistry

    What is the minimum amount of 6.6 M H2SO4 necessary to produce 22.6 g of H2 (g) according to the following reaction? 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) I need to find the volume of the H2SO4 Work: 22.6g H2 /2.008g H2 = 11.3

  4. chemistry check

    A) Write a balanced chemical equation for the reaction between sulfuric acid and potassium hydroxide. I got H2SO4 + KOH ---> H2OH + KSO4 B) Write the ionic equation for the reaction. H2 + S2O4-2 + K + OH- ---> H2 + OH + K2SO4-2 C)

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