1. Questions

Chemistry

A sample of an oxide of antimony (Sb) contained 25.0 g of antimony combined with 8.2 g of oxygen. The simplest formula for the oxide is?

  1. 👍
  2. 👎
  3. 👁
Chris

  1. Convert 25.0 g Sb to moles.
    Convert 8.2 g oxygen to moles.
    Find the ratio of one element to the other in small whole numbers. The easiest way to do that is to divide the smaller number of moles by itself. That assures a 1.000 for that numbers. Then divide the other by the same small whole number, round to whole numbers and that should be the empirical formula. [Note: In rounding to a whole number, be careful that you don't "round" too much; i.e., a 0.25 could become a whole number by multiplying everything by 4, a 0.5 could become a whole number by multiplying everything by 2, etc).

    1. 👍
    2. 👎
    DrBob222

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 problem- percent yield

    Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3 (s) + 3Fe(s) ¨ 2Sb(s) + 3FeS(s) When 15.0 g Sb2S3 reacts with an excess of Fe, 9.84 g Sb is produced. What is the

  3. chemistry

    The quantity of antimony in a sample can be determined by an oxidation-reduction titration with an oxidizing agent. A 6.35-g sample of stibnite, an ore of antimony, is dissolved in hot, concentrated HCl(aq) and passed over a

  4. Chemistry

    Freon-12 is formed as follows: 3 CCl4 + 2 SbF3 -> 3 CCl2F2 + 2 SbCl3 150 g tetra chloromethane is combined with 100 g antimony (III) fluoride to give Freon-12 (CCl2F2). Identify the limiting and excess reagents, and calculate how

  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. Chemistry

    A SAMPLE OF ANTIMONY, Ar=121.8, WAS ANALYSED AND WAS FOUND TO CONSIST OF 60% OF 121Sb AND ONE OTHER ISOTOPE. DETERMINE THE MASS NUMBER OF THE OTHER ISOTOPE IN THE SAMPLE OF ANTIMONY. please help I'm really stuck,

  3. chem

    calculate the number of moles in 0.00655 g of antimony

  4. Chemistry

    Heating an ore of antimony (Sb2S3) in the presence of iron gives the element antimony and iron(II) sulfide. Sb2S3(s) + 3Fe(s) ==> 2Sb(s) + 3FeS(s) When 15.0g Sb2S3 reacts with an excess of Fe, 9.84g Sb is produced. What is the

  1. Chemistry

    A 0.700 g sample containing Ag2O and inert material is heated, causing the silver oxide to decompose according to the following equation: 2 Ag2O(s) → 4 Ag(s) + O2(g) If 13.8 mL of gas are collected over water at 27°C and 1.00

  2. chemistry

    The difference samples A and B of Zinc oxide we're obtained from different sources when heated in a stream of hydrogen they were reduced to yield the following results ZnO. Mass of sample. Mass of Zn red. Sample. A 10.0g. 8.11g

  3. Chemistry

    The quantity of antimony in an ore can be determined by an oxidation-reduction titration with an oxidizing agent. The ore is dissolved in hot, concentrated acid and passed over a reducing agent so that all the antimony is in the

  4. chem

    . Antimony pentachloride decomposes according to the following equation. SbCl5 (g) → SbCl3 (g) + Cl2 (g) Suppose that 10.0 g of antimony pentachloride is placed in a 5.00 L container and allowed to establish equilibrium.

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