How does a chemical reaction obey the law of conservation of matter? A B C D The same number of molecules appear in the reactants as appear in the products. The total mass of the reactants is equal to the total mass of the products. The same total number of chemical bonds are in the reactants as are in the products. The same number of reactant particles as product particles are in- volved in the reaction.

How does a chemical reaction obey the law of conservation of matter? A B C D The same number of molecules appear in the reactants as appear in the products. The total mass of the reactants is equal to the total mass of the products. The same total number of chemical bonds are in the reactants as are in the products. The same number of reactant particles as product particles are in- volved in the reaction.

Introductory Chemistry: A Foundation

8th Edition

ISBN:9781285199030

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 44QAP: According to the law of conservation of mass, mass cannot be gained or destroyed in a chemical...

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Two 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.
According to the law of conservation of mass, mass cannot be gained or destroyed in a chemical reaction. Why can't you simply add the masses of two reactants to determine the total mass of product? Choose the best answer and explain. One of the reactants could be present in excess, and not all of it will be used to make the product(s). The masses of the reactants must be converted to moles first and then added. Not all chemical reactions follow the law of conservation of mass, especially ones with mixed physical states present. The masses of the two reactants cannot be added until they are each multiplied by their coefficient in the balanced equation. It is only the molar masses that are conserved in chemical reactions, not the actual mass amounts given in the laboratory.
hat do the coefficients of a balanced chemical equation tell us about the proportions in which atoms and molecules react on an individual (microscopic) basis?
Use the law of conservation of mass to determine which numbered box(es) represent(s) the product mixture after the substances in the unnumbered box undergo a reaction.
According to the law of conservation of mass, mass cannot be gained or destroyed in a chemical reaction. Why cant you simply add the masses of two reactants to determine the total mass of product?
What is true about the chemical properties of the product? a. The properties are more like chemical A. b. The properties are more like chemical B. c. The properties are an average of those of chemical A and chemical B. d. The properties are not necessarily like either chemical A or chemical B. e. The properties arc more like chemical A or more like chemical B, but more information is needed. Justify your choice, and for choices you did not pick, explain what is wrong with them.
An element X bas five major isotopes, which are listed below along with their abundances. What is the element? Isotope Percent Natural Abundance Mass (u) 46x 8.00% 45.95232 47x 7.30% 46.951764 48x 73.80% 47.947947 49x 5.50% 48.947841 50x 5.40% 49.944792
With the advent of techniques such as scanning tunneling microscopy, it is now possible to write with individual atoms by manipulating and arranging atoms on an atomic surface. a. If an image is prepared by manipulating iron atoms and their total mass is 1.05 1020 g, what number of iron atoms were used? b. If the image is prepared on a platinum surface that is exactly 20 platinum atoms high and 14 platinum atoms wide, what is the mass (grams) of the atomic surface? c. If the atomic surface were changed to ruthenium atoms and the same surface mass as determined in part b is used, what number of ruthenium atoms is needed to construct the surface?
3.112 In one experiment, the burning of 0.614 g of sulfur produced 1.246 g of sulfur dioxide as its only product. In a second experiment run to verify the outcome of the first, a sample was burned and 0.813 g of sulfur dioxide was obtained, but the student running the experiment forgot to determine the initial mass of sulfur burned. Describe how the data already obtained could be used to calculate the initial mass of the sulfur burned in the second experiment.
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.)
5 g of anhydrous strontium nitrate is added to a beaker and exposed to air. After several hours the beaker and the contents are weighed. It was found that the mass increased by 1.70 g. Assume that the increase in mass is totally due to the absorption of water by the anhydrous compound. Hoe many moles of water were absorbed by the strontium nitrate?
Which of the following is not a consequence of the Law of Conservation of Matter? It provides a basis for balancing chemical equations. It means that there will be no observable change in the quantity of matter during a chemical reaction. As a result, there will be the same number of moles on both the reactant and the product side of a balanced equation. It can be stated as “matter is neither created nor destroyed during a chemical reaction.