Two elements, R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R combines with 3.00g of Q. In the second compound, 7.00g of R combines with 4.50g of Q. Show that these data are in accord with the law of multiple proportions. If the formula of the second compound is RQ, what is the formula of the first compound?

Two elements, R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R combines with 3.00g of Q. In the second compound, 7.00g of R combines with 4.50g of Q. Show that these data are in accord with the law of multiple proportions. If the formula of the second compound is RQ, what is the formula of the first compound?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 12.6712.67 g sample of NaBr contains 22.3422.34% Na by mass. Considering the law of constant composition (definite proportions), how many grams of sodium does a 6.636.63 g sample of sodium bromide contain?
An element has the following natural abundances and isotopic masses: 78.99% abundance with 23.985 amu, 10.00% abundance with 24.986 amu, and 11.01% abundance with 25.983 amu. Calculate the weighted average atomic mass of this element. Use the correct number of significant figures in your answer. Identify the element, by name and symbol.
A combustion reaction involves the reaction of a substance with oxygen gas. The complete combustion of any hydrocarbon (binary compound of carbon and hydrogen) produces carbon dioxide and water as the only products. Heptane is a hydrocarbon that is found in gasoline. Complete combustion of heptane produces 7 liters of carbon dioxide for every 8 liters of water vapor (both measured at the same temperature and pressure). What is the ratio of carbon atoms to hydrogen atoms in a molecule of heptane?
5. Law of Multiple Proportions. Two elements, R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R combines with 3.00 g of Q. In the second compound, 7.00 g of R combines with 4.50 g of Q. Show that these data are in accord with the law of multiple proportions. If the formula of the second compound is RQ, what is the formula of the first compound?
Chromium which has an average atomic mass of 51.9961 amu has four isotopes. The masses of its isotopes are 49.94605 amu, 51.94051 amu, 52.94065 amu and 53.93888 amu. The first two isotopes have a total abundance of 87.87% and the last isotope has an abundance of 2.365%. What is the abundance of the third isotope? Answer text
A 8.63 g sample of calcium sulfide was decomposed into its constituent elements, producing 4.80 g of calcium and 3.83 g of sulfur. Which of the statements are consistent with the law of constant composition (definite proportions)? The mass percentage of calcium plus the mass percentage of sulfur in every sample of calcium sulfide equals 100%. The mass ratio of Ca to S in every sample of calcium sulfide is 1.25. Every sample of calcium sulfide will be 55.6% by mass calcium. The mass ratio of S to Ca will vary based on how the sample was prepared. A different 8.63 g sample of calcium sulfide will contain a different amount of calcium.
The average atomic mass of copper is 63.546 amu. It is composed of copper-63 and copper-65 isotopes. The natural abundance of copper-63 (62.9296 amu) is 69.17%. Show how the natural abundance of copper-65 (64.9278 amu) can be determined two different ways from the given information.
These exercises are not divided by category, although they are roughly in the order of the topics in the chapter. They are not paired. The element oxygen has three naturally occurring isotopes, with 8, 9, and 10 neutrons in the nucleus, respectively. Write the full chemical symbols for these three isotopes.Describe the similarities and differences between the three kinds of atoms of oxygen.