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Jennifer

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  • Using the Standard Enthalpies of Formation to calculate the enthalpy change for a reaction:?

    The equation for the reaction between methane and chlorine is:

    CH4(g) + 2Cl2(g) → CCl4(l) + 2H2(g)

    I'm to use the Standard Enthalpies of Formation to calculate the enthalpy change for this reaction, showing all work to complete the problem, and I'm stuck. I have a general idea, but need assistance so I can complete 9 other similar problems. Thank you.

    1 AnswerChemistry1 decade ago
  • Determining the percent yield of a reaction?

    In alcohol fermentation, yeast converts glucose to ethanol and carbon dioxide:

    C6H12O6(s) --> 2C2H5OH(l) + 2CO2(g)

    So if 6.00g of glucose are reacted and 1.44 Liters of CO2 gas are collected at 293K and 0.984 atm, I need to find the percent yield of the reaction.

    I know that, theoretically, for every one mole of glucose reacted, two moles of carbon dioxide will be produced, and using the molar mass of glucose (180.2g/mol) and the given initial mass of glucose (6.00g) I need to determine the theoretical number of moles of carbon dioxide produced, then use the ideal gas equation to determine the theoretical volume of carbon dioxide produced. However, no answer I come up with is checking out as the correct percent yield of the reaction.

    2 AnswersChemistry1 decade ago
  • What is the theoretical yield of TiO2?...?

    Titanium(IV) oxide (TiO2) is a white substance produced by the action of sulfuric acid on the mineral ilmenite (FeTiO3):

    FeTiO3+H2SO4 --> TiO2+FeSO4+H2O

    Its opaque and nontoxic properties make it suitable as a pigment in plastics and paints. In one process, 8.25 x 10^3 kg of FeTiO3 yielded 3.62 x 10^3 kg of TiO2.

    I know the following:

    The molar mass of FeTiO3 is 151.73 g (or g/mol).

    The molar mass of TiO2 is 79.88 g (or g/mol).

    The balanced equation shows a mole ratio of 1 mole TiO2 : 1 mole FeTiO3.

    Two things:

    1) What is the percent of the reaction?

    2) What is the theoretical yield of TiO2?

    Please, if possible, don't just give the answer. I'm stumped and need to know how the answer was obtained as well. Thanks!

    1 AnswerChemistry1 decade ago