Ask Question
24 December, 23:55

Examine the following unbalanced equation.

HCl (g) + O2 Cl2 (g) + H2O (g)

Assuming that all the gases in this reaction are at STP, what number of molecules of hydrogen chloride gas are needed to completely react with oxygen to yield 50.00 mL of chlorine gas?

+1
Answers (1)
  1. 24 December, 23:59
    0
    1) Determine the number of moles of chlorine gas

    At STP 1 mol = 22.4 liter

    => [1mol/22.4 liter] * 0.050 liter = 0.00223 mol Cl2 (g)

    2) Write the balanced equation

    4HCl (g) + O2 - - > 2Cl2 (g) + 2H2O (g)

    3) Write the ratios of the compound on which you are focused.

    4 HCl : 2 mol Cl2

    Then, 0.00223 mol Cl2 * [4mol HCl / 2 mol Cl2] = 0.00446 mol HCl

    5) Use Avogadro's number to find the number of molecules:

    0.00446 mol * 6.02*10^23 = 2.68 * 10^21 molecules of HCl

    Answer: 2.68 * 10^21 molecules
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Examine the following unbalanced equation. HCl (g) + O2 Cl2 (g) + H2O (g) Assuming that all the gases in this reaction are at STP, what ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers