Consider the following reaction.
SO3(g) + H2O(l) → H2SO4(aq)

A chemist allows 60.9 g of SO3 and 11.1 g of H2O to react. When the reaction is finished, the chemist collects 54.4 g of H2SO4. Determine the limiting reactant, theoretical yield, and percent yield for the reaction

  1. 👍
  2. 👎
  3. 👁
  1. mols SO3 = grams/molar mass = ?
    mols H2O = grams/molar mass = ?

    Using the coefficients in the balanced equation, convert mols SO3 to mols H2SO4.
    Do the same and convert mols H2O to mols H2SO4.
    In limiting reagent problems the SMALLER amount of product formed is ALWAYS the right correct answer and the reagent responsible for that is the limiting reagent.
    Then grams H2SO4 = mols H2SO4 x molar mass H2SO4. The is the theoretical yield(TY). The actual yield (AY) in the problem is 54.4 g.
    % yield = (AY/TY)*100 = ?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    For the reaction, 2SO2(g) + O2(g) ¨ 2SO3(g) + heat, at equilibrium, what will be the effect on the net amount of SO3 present if the temperature of the container is increased? A) The concentration of SO3 decreases. B) The

  2. Chemisty

    For the reaction SO3 plus H2O>>H2SO4, calculate the percent yield if 500.g of sulfur trioxide react with excess water to produce 575g of sulfuric acid??

  3. Chemistry

    H2SO4(aq) + H2O(l) ⟶ H3O+(aq) + HSO4–(aq) (Stage I) Identify the Brønsted-Lowry acid and base in the reaction.

  4. Chemistry

    Predict the product(s) for the following reaction: H2SO4(aq) + KOH(aq) --> Choose one answer. a. K(s) + H2(g) + SO3(g) b. K2SO4(aq) + H2O(l) c. No reaction occurs d. K2S(aq) + H2O(l) e. KSO4(aq) + H2O(l) I keep getting: K2SO4(aq)

  1. Chemistry

    Classify each of the following as a redox reaction or a non-redox reaction. Zn+CuCl2 -> ZnCl2+Cu HCl+NaOH -> H2O+NaCl 2CO+O2 -> 2CO2 SO3+H2O -> H2SO4

  2. chemistry

    When 25.0 mL of 1.0 M H2SO4 is added to 50.0 mL of 1.0 M NaOH at 25.0 °C in a calorimeter, the temperature of the aqueous solution increases to 33.9 °C. Assuming the specific heat of the solution is 4.18 J/(g·°C), that its

  3. Chemistry

    What would be more acidic? SO2 or SO3? Does this have to do something with the higher oxidation state? And why is that? Or can we say SO3 is more acidic by, SO2+H2O--->H2SO3 SO3+H2O--->H2SO4 as H2SO4 is more acidic?

  4. chemistry

    Which of the following is a precipitation reaction? I. 2 Mg (s) + O2 (g) → 2 MgO (s) II. SO3 (g) + 2 H2O (l) → H3O+ (aq) + HSO4- (aq) III. Pb2+ (aq) + CrO42- (aq) → PbCrO4 (s) IV. 2 H2O (g) → 2 H2 (g) + O2 (g) V. Ag+ (aq)

  1. Chem

    Which of the following is not an example of a neutralization reaction? A HCl + NaOH NaCl +H2O B 2 NaOH + H2CO3 Na2CO3 +2 H2O C H2SO4 + 2 NH4OH (NH4)2SO4 + 2 H2O D 2 AgNO3 + Zn 2Ag +Zn(NO3)2 A?

  2. Chemistry

    I don't understand this question? What is the maximum amount in grams of SO3 that can be produced by the reaction 1.0 g of S with 1.0 g of O2 EQUATION: 2 S(s) +3 O2(g)--->2 SO3(g) The choices are: A) 3.8 B) 2.5 C) 0.27 D) 1.7

  3. Chemistry

    Sulfur trioxide, SO3, is made from the oxidation of SO2, and the reaction is represented by the equation 2SO2 + O2 2SO3 A 25-g sample of SO2 gives 18 g of SO3. The PERCENT YIELD of SO3 is?

  4. chemistry (Pls Bob check for me)

    A 0.5g of fuming h2so4 oleum is diluted with water. This solution is completedly neutralized by 26.7ml of 0.4N naoh. Find the percentage of free so3 in the sample The asnwer 20.6% My calculation h2so4= 98/2 = 49 so3= 80/2 = 40

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