Chemistry

For each of the following unbalanced equations, suppose that exactly 15.0g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of each product is expected. assume the limiting reactant is completely consumed.
a)Al+HCL->AlCl3+H2
b)NaOH+CO2->Na2CO3+H2O
c)Pb(NO3)2+HCL->PbCl2+HNO3
d)K+I2->KI

  1. 👍 0
  2. 👎 0
  3. 👁 1,814
  1. Write the balanced equation.
    2Al + 6HCl ==> 2AlCl3 + 3H2

    Convert 15.0 g Al to moles.
    Convert 15.0 g HCl to moles.
    15.0 g Al x (1 mole Al/26 g) = 0.555
    15.0 g HCl x (1 mole HCl/36.5 g) = 0.410

    Convert moles of each to mols of either product (but stay consistent). Let's choose AlCl3.
    0.555 moles Al x (2 moles AlCl3/2 moles Al) = 0.555 x 1/1 = 0.555 moles AlCl3.

    0.410 moles HCl x (2 moles AlCl3/6 moles HCl) = 0.410 x 2/6 = 0.137 moles AlCl3.

    The SMALLER number of moles produced by the HCl means two things: (a) HCl is the limiting reagent, and (b)0.137 moles AlCl3 is the amount of product formed using 15.0 g of each reactant initially.

    Now convert moles AlCl3 to grams.
    0.137 moles AlCl3 x (133.5 g AlCl3/1 mole AlCl3) = 18.3 g.

    All of the problems are worked this way. Just follow this template. And you need to redo this one from the beginning for two reasons. First, I estimated the atomic masses and molar masses and you need to use the exact values to obtain a correct answer. Second, you need the practice and this can be a good practice problem because you know the answers for each step.

    1. 👍 1
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    MnO4–(aq) + Cl–(aq) Mn2+ + Cl2(g) (unbalanced) i. Write the reduction and oxidation half-reactions (without electrons). (.5 point) ii. Balance the equations for atoms (except O and H). (.5 point) iii. Balance the equations for

  2. chemistry

    2H2O2 --- 2H2O + O2 is this a redox reaction if so what is the oxidized reactant and reduced reactant

  3. chemistry

    Where possible, classify these systems as reactant-favored or product-favored at 298 K. If the direction cannot be determined from the information given, classify the reaction as "Insufficient information". a)2A(g) + 3B(g)

  4. science

    Consider the equation: CH4+O2→2H2O+CO2 Which element or elements are unbalanced in this equation? A- Both H and O are unbalanced. B- C, H, and O are all unbalanced. C- Only the O is unbalanced. D- Only the H is unbalanced.

  1. chemistry

    Consider the unbalanced reaction Ti(s) + Cl2(g) --> TiCl4(s) When 10.3 g of Ti react with 12.7 g of Cl2, 16.2 g of TiCl4 are obtained. The theoretical yield of TiCl4 is , the limiting reactant is and the percent yield is %.

  2. chemistry

    Calculate how many grams of the first reactant are necessary to completely react with 55.8g of the second reactant. Na2CO3 + CuCl2 → CuCO3 + 2 NaCl

  3. Chem

    For each unbalanced equation below, calculate how many grams of each product would be produced by complete reaction of 12.5g of the reactant indicated. Indicate clearly the mole ratio used for the conversion. A.

  4. physical

    staring from rest, a 3.5 kg object is acted upon by an unbalanced force and acquires a speed of 14.0 m/s after moving a distance of 35 m. find (a) the acceleration of the object, (b) the unbalanced force acting on the object, and

  1. chemistry

    How many of the following are true concerning balanced chemical equations? I. The number of molecules is conserved. II. The coefficients for the reactants tell you how much of each reactant you are given. III. Atoms are neither

  2. Chemistry

    For each of the following precipitation reactions calculate how many grams of the first reactant are necessary to completely react with 55.8 g of the second reactant. K2SO4 + Sr(NO3)2 + SrSO4 + 2KNO3

  3. Chemistry

    Iron is obtained from iron ore according to the following reaction: Fe2O3+CO---> Fe+CO2 (unbalanced). a. Assuming the blast furnace is 90.0% efficient in recovering the iron, what is the actual mass of iron obtainable from a ton

  4. Chemistry

    If K > 1 at 25°C and 1 atm of pressure, then which statement is true about the reaction's equilibrium? A. There is always more reactant than product at equilibrium under all conditions. B. There is more product than reactant at

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