Open Question
Calculate the density of a liquid in g/mL to the correct number of significant digits, if a flask containing 9.55 mL of the liquid weighs 157.2 g with the liquid and 148.4 g when empty.
Ch.1 - Matter, Measurement & Problem Solving
Chapter 1, Problem 35
A chemist decomposes several samples of carbon monoxide into carbon and oxygen and weighs the resultant elements. The results are shown in the table. Do you notice a pattern in these results? Next, the chemist decomposes several samples of hydrogen peroxide into hydrogen and oxygen. The results are shown in the table. Do you notice a similarity between these results and those for carbon monoxide? Can you formulate a law from your observations? Can you formulate a hypothesis that might explain your law?
Verified step by step guidance1
<insert step 1: Begin by examining the data provided for the decomposition of carbon monoxide (CO) into carbon (C) and oxygen (O). Note the masses of carbon and oxygen obtained from each sample.>
<insert step 2: Calculate the ratio of the mass of oxygen to the mass of carbon for each sample of carbon monoxide. This will help identify any consistent pattern.>
<insert step 3: Repeat the process for the decomposition of hydrogen peroxide (H2O2) into hydrogen (H) and oxygen (O). Calculate the ratio of the mass of oxygen to the mass of hydrogen for each sample.>
<insert step 4: Compare the ratios obtained from the decomposition of carbon monoxide and hydrogen peroxide. Look for any similarities or consistent patterns in the ratios.>
<insert step 5: Based on the observed patterns, formulate a law that describes the relationship between the elements in the compounds. Consider proposing a hypothesis that could explain the observed law, such as the Law of Definite Proportions, which states that a chemical compound always contains its component elements in fixed ratio by mass.>
Related Practice
Textbook Question
Classify each statement as an observation, a law, or a theory. a. All matter is made of tiny, indestructible particles called atoms. b. When iron rusts in a closed container, the mass of the container and its contents does not change. c. In chemical reactions, matter is neither created nor destroyed. d. When a match burns, heat is released
755
views
Textbook Question
Classify each statement as an observation, a law, or a theory. a. Chlorine is a highly reactive gas. b. If elements are listed in order of increasing mass of their atoms, their chemical reactivities follow a repeating pattern. c. Neon is an inert (or nonreactive) gas. d. The reactivity of elements depends on the arrangement of their electrons.
940
views
Open Question
Can you devise a hypothesis to explain why most distant galaxies are moving away from each other, and why the more distant galaxies are moving away more rapidly?
Textbook Question
Classify each substance as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous. a. sweat b. carbon dioxide c. aluminum d. vegetable soup
2914
views
Textbook Question
Classify each substance as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous. a. wine b. beef stew c. iron d. carbon monoxide
2497
views