Chemistry

Assuming an efficiency of 38.60%, calculate the actual yield of magnesium nitrate formed from 145.9 g of magnesium and excess copper(II) nitrate.
I got 230.5g but it isn't right..
I got 6 mols of Mg then calculated molar mass of Mg(NO3)2 and got 148.31 and then multiplied the two together
Then I used the percent yield given to find the actual yield.

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
  1. Mg + Cu(NO3)2 ==> Mg(NO3)2 + Cu
    mols Mg = 145.9/24.3 = 6.003
    The equation is 1 mol to 1 mol; therefore, you will have 6.003 mol Mg(NO3)2 formed. Molar mass I have is 148.31 to give g Mg(NO3)2 =890.29g at 100% yield.
    890.29 x 0.3860 = 343.65g actual yield. You're allowed 4 s.f. and I would round to 343.6g.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
  2. Thank you!

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    magnesium powder reacts with steam to form magnesium hydroxide and hydrogen gas. What is the pecentage yield of 10.1g Mg reacts with an excess of water abnd 21.0g Mg 9g (OH)2 is recovered? If 24g Mg is used the percentage yield is

  2. Chemistry

    According to his prelaboratory theoretical yield calculations, a student's experiment should have produced 1.44 g of magnesium oxide. When he weighed his product after reaction, only 1.23 g of magnesium oxide was present. what is

  3. Chemistry (Stoichiometry)

    Magnesium powder reacts with steam to form magnesium hydroxide and hydrogen gas. a) Write a balanced chemical equation for this reaction. b) What is the percentage yield if 10.1g Mg reacts with an excess of water and 21.0g Mg(OH)2

  4. chem

    What is the actual amount of magnesium oxide produced when excess carbon dioxide reacts with 42.8 g of magnesium metal? The percent yield of MgO(s)for this reaction is 81.7%. 2Mg(s) . CO2(g) y 2MgO(s) . C(s)

  1. chemistry

    Magnesium nitride is formed in the reaction of magnesium metal with nitrogen gas in this reaction: 3 Mg(s) + N2(g) --> Mg3N2(s) How many grams of product are formed from 2.0 mol of N2 (g) and 8.0 mol of Mg(s)? i havent been able

  2. Chemistry

    4 Fe + 3 O2 -> 2 Fe2O3 1. If I react 3.00g Fe and 5.75g O2, what is the theoretical yield? 2. If I’m only able to produce 3.5g, what is my percent yield? 3. If I try again, and get a 95.0% yield, what is my actual yield? For the

  3. Chemistry

    Consider the following chemical equation: TiCl4(g) + 2Mg(l) → Ti(s) + 2MgCl2(l) 3.54×107g of TiCl4(g) were reacted completely and 7.91×106g of Ti(s) was obtained in the experiment. a. Calculate the theoretical yield of Ti(s).

  4. chemistry

    When aqueous solutions of potassium carbonate and magnesium nitrate are combined, solid magnesium carbonate and a solution of potassium nitrate are formed. The net ionic equation for this reaction is:

  1. chemistry

    Ammonium nitrate is used in explosives and is produced from the reaction of ammonia and nitric acid. If 15 kg of ammonia give an actual yield of 65.3 kg of ammonium nitrate, what is the percent yield? The calculated yield of

  2. stoichiometry

    if 5.00g magnesium is combined with 10.0 g of chlorine, show by calculation which substance is the limiting reactant and calculate the theoretical yield of magnesium chloride for the reaction. Someone PLEASE HELP ME!!!!

  3. Chemistry

    In a reaction 2 moles of CH4 were reacted with an excess of Cl2. As a result 117gram of CCl4 is obtained. What is theoratical yield? Actual yield? %age yield?

  4. Jim

    I need some help with calculating percent yield and percent purity of aspirin. Here's my data (questions follow): SYNTHESIS Mass of salicylic acid.., 2.0 g Volume of acetic anhydride.., 5 mL Mass of watch glass.., 22.10 g Mass of

View more similar questions or ask a new question.