1. Fill in the blanks with the most appropriate term: A are the tells the story of a chemical reaction. starting substances in the reaction while numbers in front of some of the formulas are called are the new substances that are formed. The large These numbers are used to of Mass. The number of atoms because mass cannot be the equation because chemical reactions must obey the Law of_ of each element on both sides of the equation must be When balancing equations, the only numbers that can be changed are must never be changed to balance an equation. or remember that

1. Fill in the blanks with the most appropriate term: A are the tells the story of a chemical reaction. starting substances in the reaction while numbers in front of some of the formulas are called are the new substances that are formed. The large These numbers are used to of Mass. The number of atoms because mass cannot be the equation because chemical reactions must obey the Law of_ of each element on both sides of the equation must be When balancing equations, the only numbers that can be changed are must never be changed to balance an equation. or remember that

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 9CR

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You have two distinct gaseous compounds made from element X and element Y. The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react gas X with gas Y to make the products, you get the following data (all at the same pressure and temperature): 1 volume gas X + 2 volumes gas Y 2 volumes compound I 2 volumes gas X + 1 volume gas Y 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
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.
You may have noticed that when water boils, you can see bubbles that rise to the surface of the water. Which of the following is inside these bubbles? Explain. a. air b. hydrogen and oxygen gas c. oxygen gas d. water vapor e. carbon dioxide gas
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?
Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 mole ratio and a sample of water vapor? Explain.
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.
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?
Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 ratio and a sample of water vapor? Explain.
Imagine you mix 16.05 g of methane (CH4) gas and 96.00 g ofoxygen (O2) gas and then ignite the mixture. After a bright flashand a loud bang, some water droplets form on the inside of thereaction vessel.a. Write the balanced chemical reaction for the combustion ofmethane.b. Depict the process that occurred in the vessel using circles torepresent atoms. Represent carbon with black circles, hydrogenwith white circles, and oxygen with gray circles. Let onecircle (or one molecule made of circles bonded together) representexactly one mole.c. How many moles of water can you make? How many molesof carbon dioxide?d. Will anything be left over? What? How much?e. Identify the following: limiting reagent, excess reagent, andtheoretical yield.
Say which atom is the Cl and the O His bonded with for reactants and products it is for number 19
You have two distinct gaseous compounds made from element X and element Y.The mass percents are as follows: Compound I: 30.43% X, 69.57% Y Compound II: 63.64% X, 36.36% Y In their natural standard states, element X and element Y exist as gases. (Monatomic? Diatomic? Triatomic? That is for you to determine.) When you react "gas X" with "gas Y" to make the products, you get the following data (all at the same pressure and temperature): 1 volume "gas X" + 2 volumes "gas Y" → 2 volumes compound I 2 volumes "gas X" + 1 volume "gas Y" → 2 volumes compound II Assume the simplest possible formulas for reactants and products in the chemical equations above. Then, determine the relative atomic masses of element X and element Y.
The Law of Conservation of Mass states that matter is not gained or lost in a chemical reaction. Which of the following correctly restates this law? In a chemical reaction Matter is gained and lost but energy is conserved. The amount of mass is equal to the sum of the reactants and products. Matter is gained and lost in depending on how much energy is added. The amount of mass of the reactants will equal the mass of the products