Copper metal reacts with concentrated nitric acid according to the following balanced equation:

3Cu(s) + 8HNO3(aq) �¨ 3Cu(NO3)2(s) + 2NO(g) + 4H2O(l)

Calculate the mass in grams of the excess reagent remaining after the complete reaction of 4.63 g of Cu with 9.26 g of HNO3. Round your answer to 2 decimal places.

  1. 0
  2. 0
  3. 5
asked by Hector
  1. 1. You have the balanced equation.
    2. Convert g Cu to mols Cu.
    3. Convert g HNO3 to mols HNO3.
    4a. Convert mols Cu to mols Cu(NO3)2.
    4b. Convert mols HNO3 to mols Cu(NO3)2.
    4c. Choose the smaller mols of Cu(NO2)2 2. The reagent producing that number (either 4a or 4b) will be the limiting reagent.
    5. Convert mols of the limiting reagent to mols of the other reagent. That will be how much of the other reagent (the excess reagent) is used.
    6. Convert mols of the excess reagent used to grams, subtract from the initial mass present, and that will give you the amount remaining after reaction.
    Post your work if you need more help.

    1. 0
    2. 0
    posted by DrBob222
  2. 89

    1. 0
    2. 0
    posted by lo

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    copper metal reacts with nitric acid. assume that the reaction is 3Cu(s) + 8HNO3(aq) ——> 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l). if 5.58 grams of Cu(NO3)2 is obtained, how many grams of nitrogen monoxide would have formed
  2. Chemisty

    A 0.411 g sample of powdered copper mixed with an inert, soluble additive was fully consumed by 23.4mL of 0.602M nitric acid, producing copper (II) nitrate, water, and nitric oxide. What is the percent copper by mass in the
  3. Chemistry

    1) A double displacement reaction takes place when aqueous sodium carbonate reacts with aqueous tin (II) nitrate. You would expect one of the products of this reaction to be. Answer: Sn(CO3)2 2) For the reaction, 3 Cu + 8HNO3 -->
  4. Chemistry

    3Cu(s) + 8HNO3(aq) → 2NO(g) + 3Cu(NO3)2(aq) + 4H2O(l) If 15 g of copper metal was added to an aqueous solution containing 6.0 moles of HNO3, how many moles of NO(g) would be produced, assuming a 59.8 % yield.
  5. Chemistry

    Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper (II) sulfate, sulfur dioxide gas and water. What type of reaction is this?
  6. Chemistry

    Students are instructed to add no more than 0.25 mL of 15 M nitric acid. What volume of 15 M nitric acid is required to react with 0.030 g of copper metal? If 1.0 mL of acid contains approximately 20 drops, how many drops of
  7. Chemistry

    1. When solid copper metal reacts with nitric acid, the products include copper (II) ion and nitrogen monoxide gas. If 11.99 g of solid copper are reacted with 153 mL of 0.322 M HNO3, how many liters of nitrogen monoxide will be
  8. Chemistry

    ammonia gas reacts with copper (ii) oxide at high temperatures to produce elemental nitrogen, copper metal, and water vapor. Assume that 36.2g ammonia reacts with 180.8 g copper ii oxide. (balanced equation: 2 NH4 (ammonium) (g) +
  9. chemistry-chemical equations

    How do I write the balanced chemical equation for Copper +nitric acid -> copper(II)nitrate+ nitrogen dioxide + water
  10. Chemistry

    True or False? a) wet metallic copper can be rinsed with acetone to help any remaining cation to metal reduction occur b)copper metal is readily oxidized by nitric acid to yield copper(II) nitrate

More Similar Questions