Chemistry

The steps to getting the answer.

A certain metal oxide has the formula MO where M denotes the metal. A 39.46g sample of the compound is strongly heated in an atmosphere of hydrogen to remove oxygen as water molecules. At the end, 31.70g of the metal is left over. If O has an atomic mass of 16.00 amu, calculate the atomic mass of M and identigy the element.

For this question the answers where Atomic Mass: 65.4 amu and element: Zn

but I don't know how to solve this.

My textbook doesn't have any examples like this question.

  1. 👍 0
  2. 👎 0
  3. 👁 1,421
  1. Use proportions.
    The mass of the oxide before and after reduction contain the same amount of metal. The masses are proportional to the sum of the AMU's:
    (M+16)/M = 39.46/31.7
    Cross multiply to get
    31.7(M+16) = 39.46M
    Solve for M to get
    M=64.87
    which lies between Cu at 63.55 and Zn at 65.39.
    Margin of error required if the metal is Zn: (65.39-64.87)/65.39= 0.8%
    which could be acceptable depending on the laboratory conditions.

    1. 👍 0
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    A 15.27 g sample of Mo2O3(s) is converted completely to another molybdenum oxide by adding oxygen. The new oxide has a mass of 18.33 g. Add subscripts below to correctly identify the empirical formula of the new oxide.

  2. chem

    A 2.241 g sample of nickel reacts with oxygen to form 2.852 g of the metal oxide. Calculate the empirical formula of the oxide. 1)NiO Give the number of moles of each element to support you answer. moles of Ni 2) 1.339 mol moles

  3. chemistry

    Tin metal is heated with oxygen gas to yield tin(IV) oxide. Express your answer as a chemical equation. Identify all of the phases in your answer

  4. Chemistry

    A particular metallic element, M, has a heat capacity of 0.36 J*g*K, and it forms an oxide that contains 2.90 grams of M per gram of oxygen. (a) Using the law of Dulong and Petit (Cp x M = 25 J*mol*K), estimate the molar mass of

  1. Chemistry

    A sample of an oxide of antimony (Sb) contained 51.5 g of antimony combined with 16.9 g of oxygen. What is the simplest formula for the oxide?

  2. Science/ Chemistry

    When 0.422 g of phosphorus is burned, 0.967 g of a white oxide (a compound of phosphorus and oxygen) is obtained. a. Determine the empirical formula of the oxide. So for the empirical Formula I got P_2O_5 now it wants me to Write

  3. chem

    A 2.241 g sample of nickel reacts with oxygen to form 2.852 g of the metal oxide. Calculate the empirical formula of the oxide. Give the number of moles of each element to support you answer.

  4. Chemistry

    In the experiment 0.500 g of copper reacted with oxygen to give 0.563 g of copper oxide. What is the empirical formula of the oxide expressed as a chemical formula?

  1. Chemistry please help

    Elemental mercury was first discovered when a mercury oxide was decomposed with heat, forming mercury metal and oxygen gas. When a 0.204-g sample of the mercury oxide is heated, 0.189 g of mercury metal remains. a)what is mole

  2. Chemistry

    When 6.25grams of pure iron are allowed to react with oxygen, a black oxide forms. If the products weighs 8.15g, what is empirical formula of the oxide?

  3. Chemistry

    Bauxite ore contains aluminum oxide Al2O3(s) which is decomposed using electricity to produce aluminum metal and oxygen gas. What mass of aluminum metal can be procuced from 155g of aluminum oxide?

  4. Chemistry

    An unknown metal, m, forms an ionic compound with the formula, M2S3. Which formula represents the compound formed by the metal with oxygen? a) MO b) MO2 c) MO3 d) M2O3

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