Gay-Lussac's law of combining volumes states that the volumes of reactants and products are in small whole-number ratios. Which of the following is NOT an assumption for the law of combining volumes? All of these are assumed for the law of combining volumes. The products and reactants must all be at the same pressure. The products and reactants must all be gases. The products and reactants must all be at the same temperature.

Gay-Lussac's law of combining volumes states that the volumes of reactants and products are in small whole-number ratios. Which of the following is NOT an assumption for the law of combining volumes? All of these are assumed for the law of combining volumes. The products and reactants must all be at the same pressure. The products and reactants must all be gases. The products and reactants must all be at the same temperature.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 69CP: You have two distinct gaseous compounds made from element X and element Y. The mass percents are as...

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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 Y2 volumes compound I 2. volumes gas X + 1 volume gas Y2 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.
Is there a difference between a homogeneous mixture of hydrogen and oxygen in a 2:1 ratio and a sample of water vapor? Explain.
62 Ammonium dinitramide (ADN), NH4N(NO2)2, was considered as a possible replacement for aluminium chloride as the oxidizer in the solid fuel booster rockets used to launch the space shuttle. When detonated by a spark, AND rapidly decomposes to produce a gaseous mixture of N2,O2, and H2O. (This is not a combustion reaction. The ADN is the only reactant.) The reaction releases a lot of heat, so the gases are initially formed at high temperature and pressure. The thrust of the rocket results mainly from the expansion of this gas mixture. Suppose a 2.3-kg sample of ADN is denoted and decomposes completely to give N2,O2, and H2O. If the resulting gas mixture expands until it reaches a temperature of 100°C and a pressure of 1.00 atm, what volume will it occupy? Is your answer consistent with the proposed use of ADN as a rocket fuel?
Cyclopropane mixed in the proper ratio with oxygen can be used as an anesthetic. At 755 mm Hg and 25C, it has a density of 1.71 g/L. (a) What is the molar mass of cyclopropane? (b) Cyclopropane is made up of 85.7% C and 14.3% H. What is the molecular formula of cyclopropane?
Suppose that you are closing a cabin in the north woods for the winter and you do not want the water in the toilet tank to freeze. You know that the temperature might get as low as 30. C, and you want to protect about 4.0 L water in the toilet tank from freezing. Calculate the volume of ethylene glycol (density = 1.113 g/mL; molar mass = 62.1 g/mol) you should add to the 4.0 L water.
58 Magnesium will burn in air to form both Mg3N2 and MgO. What mass of each product would be found if burning a 3.11-g sample of magnesium to completion produces a combined total of 5.09 g of the two products?
In an experiment, sulfuric acid reacted with different volumes of sodium thiosulfate in water. A yellow precipitate was formed during the reaction. A cross drawn at the base of each flask became gradually invisible due the formation of this yellow precipitate. The time taken for the cross to become invisible was recorded. A partial record of the experiment is shown. Experimental Record Flask Volume ofH2SO4 Volume ofSodium Thiosulfate Volume ofWater Time 1 5 mL 50 mL 0 mL 19 seconds 2 5 mL 40 mL 10 mL 3 5 mL 30 mL 20 mL 4 5 mL 20 mL 30 mL Based on your knowledge of factors that affect the rates of chemical reactions, predict the trend in the last column of the experimental record. Use complete sentences to explain the trend you predicted. You do not have to determine exact values for time; just describe the trend you would expect (increase or decrease) and why it occurs.
Nitroglycerin (C3H5N3O9) is a powerful explosive. Its decomposition may be represented by 4C3H5N3O9 ⟶ 6N2 + 12CO2 + 10H2O + O2 This reaction generates a large amount of heat and many gaseous products. It is the sudden formation of these gases, together with their rapid expansion, that produces the explosion. (a) What is the maxi- mum amount of O2 in grams that can be obtained from 2.00 × 102 g of nitroglycerin? (b) Calculate the percent yield in this reaction if the amount of O2 generated is found to be 6.55 g.
1.The following results have been obtained for the density of nitrous oxide in grams per liter at several pressures at 0°C: 1 1.9804 2/3 1/2 Pressure (atm) Density 1.3164 0.9861 Determine the molecular weight of nitrous oxide and the atomic weight of Nitrogen. 1/3 0.6565
Using the moles of Locust Carbonate calculated in the question above, calculate the volume of gas produced in the reaction with Locust Carbonate. Assume the gas behaves ideally and you are at standard temperature (T=293 K) and pressure (P=1.0 atm). Given that the total volume of gas produced in the complete reaction (both reactions combined) is 0.500 L, calculate the mass of Quakerium in the sample (Assume Qu is 34.02 g/mol and you are at standard temperature (T=293 K) and pressure (P=1.0 atm)).
Solid copper(II) chloride forms a hydrate of formula CuCl2 ⋅ xH2O. A student heated a sample of hydrated copper(II) chloride, in order to determine the value of x. The following results were obtained: mass of crucible = 16.221 g mass of crucible and hydrated copper(II) chloride = 18.360 g mass of crucible and anhydrous copper(II) chloride = 17.917 g At. Mass: Cu 63.55 Cl 35.45 H 1.008 O 16.00 1. Calculate the number of moles of H2O (answer must be expressed to 5 decimal places)
Solid copper(II) chloride forms a hydrate of formula CuCl2 ⋅ xH2O. A student heated a sample of hydrated copper(II) chloride, in order to determine the value of x. The following results were obtained: mass of crucible = 16.221 g mass of crucible and hydrated copper(II) chloride = 18.360 g mass of crucible and anhydrous copper(II) chloride = 17.917 g At. Mass: Cu 63.55 Cl 35.45 H 1.008 O 16.00 1. Calculate the number of moles of anhydrous copper(II) chloride (answer must be expressed to 5 decimal places)