Introductory Chemistry For Today
8th Edition
ISBN: 9781285644561
Author: Seager
Publisher: Cengage
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200 g of a silicon compound is decomposed, resulting in 41 g of solid silicon and the remainder of some gas which was not weighed. Based on this information, which of the following compounds was decomposed, SiClF3 or SiCl2H2, or could it be either one?
2.90 grams of phosphorus is burned in the presence of oxygen and forms 5.14 grams of a phosphorus oxide. What is the emperical formula of the phosphorus oxide formed? Then write a balanced equation for the formation of the phosphorus oxide.
5.00 g of copper is reacted with 5.00 g of sulfur in a crucible and acompound composed of copper and sulfur is formed. If the copper was completely reacted and the mass of the compound is 6.26 g, how many grams of sulfur formsthe compound? Calculate the mass percentage of copper and sulfur, respectively, in the compound.
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- These questions concern the work of J. J. Thomson: From Thomson’s work, which particles do you think he would feel are most important in the formation of compounds (chemical changes) and why? Of the remaining two subatomic particles, which do you place second in importance for forming compounds and why? Come up with three models that explain Thomson’s findings and evaluate them. To be complete you should include Thomson’s findings.arrow_forwardTwo basic laws of chemistry are the law of conservation of mass and the law of constant composition. Which of these laws (if any) do the following statements illustrate? (a) Lavoisier found that when mercury(ll) oxide, HgO, decomposes, the total mass of mercury (Hg) and oxygen formed equals the mass of mercury(ll) oxide decomposed. (b) Analysis of the calcium carbonate found in the marble mined in Carrara, Italy, and in the stalactites of the Carlsbad Caverns in New Mexico gives the same value for the percentage of calcium in calcium carbonate. (c) Hydrogen occurs as a mixture of two isotopes, one of which is twice as heavy as the other.arrow_forwardEstimating the radius of a lead atom. (a) You are given a cube of lead that is 1.000 cm on each side. The density of lead is 11.35 g/ cm3. How many atoms of lead are in the sample? (b) Atoms are spherical; therefore, the lead atoms in this sample cannot fill all the available space As an approximation, assume that 60% of the space of the cube is filled with spherical lead atoms. Calculate the volume of one lead atom from this information. From the calculated volume (V) and the formula (4/3) 3 for the volume of a sphere, estimate the radius (r) of a lead atom.arrow_forward
- In 1886 Eugene Goldstein observed positively charged particles moving in the opposite direction to electrons in a cathode ray tube (illustrated below). From their mass, he concluded that these particles were formed from residual gas in the tube. For example, if the cathode ray tube contained helium, the canal rays consisted of He+ ions. Describe a process that could lead to these ions. Canal rays. In 1886, Eugene Goldstein detected a stream of particles traveling in the direction opposite to that of the negatively charged cathode rays (electrons). He called this stream of positive particles "canal rays:"arrow_forwardFrom the information given above, indicate onechemicalproperty of magnesium metal.arrow_forwardExplain the termselement, afoul, and compound. Provide an example and microscopic drawing of each.arrow_forward
- A jar contains some number of jelly beans. To find out precisely how many are in the jar, you could dump them out and count them. How could you estimate their number without counting each one? (Chemists need to do just this kind of bean counting when they work with atoms and molecules. Atoms and molecules are too small to count one by one, so chemists have worked out other methods to determine the number of atoms in a sample.)arrow_forwardThe density of a mixture of gases may be calculated by summing the products of the density of each gas and the fractional volume of space occupied by that gas. (Note the similarity to the calculation of the molar mass of an element from the isotopic masses and fractional abundances.) Assume dry air with CO2 removed is 20.96% (by volume) oxygen. 78.11% nitrogen, and 0.930% argon. Determine the density of argon.arrow_forwardWhat is acompound? What are compounds composed of? What is true about the composition of a compound, no matter where we happen to find the compound?arrow_forward
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