Oxygen gas can be prepared by heating potassium chlorate according to the following equation:2KCIO3(s)2KCI(s) +302(g)The product gas, O, is collected over water ata temperature of 25 C and a pressure of 749 mm Hg. If the wet O, gas formed occupies a volume of 5.55 L, thenumber of moles of KC1O3 reacted wasmol. The vapor pressure of water is 23.8 mm Hg at 25 °C

The given reaction is shown below.

Answered: Oxygen gas can be prepared by heating…

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...

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Consider the following situation: You have a 50 L tank of compressed air at 15 atm and 100 ºC. You then pass the compressed air through a "titanium getter" which contains fragments of hot titanium metal. The purpose of the "getter" is to remove oxygen gas from the sample as Ti reacts with oxygen to form solid TiO2 (known as titania). Once the purified air is passed through the getter is it cooled back down to 100 ºC and fills another 50 L storage tank. If air typically contains about 20% oxygen, what could the pressure in the storage tank be? Question 2 options: A) 12 atm B) 15 atm C) 18 atm D) 24 atm
The generic reaction occurs in a closed container:A(g) + 2 B(g) -----> 2 C(g) A reaction mixture initially contains 1.5 L of A and 2.0 L of B. Assuming that the volume and temperature of the reaction mixture remain constant, what is the percent change in pressure if the reaction goes to completion?
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For many purposes we can treat propane (C,Hg) as an ideal gas at temperatures above its boiling point of -42. °C. Suppose the temperature of a sample of propane gas is raised from -20.0 °C to 21.0 °C, and at the same time the pressure is changed. If the initial pressure was 1.5 atm and the volume increased by 35.0%, what is the final pressure? Round your answer to 2 significant digits. atm x10
A sample of nitrogen gas was collected via water displacement. Since the nitrogen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 21 °C is 1.77 atm, what is the partial pressure of nitrogen? The vapor pressure of water at 21 °C is 18.7 mm Hg. atm PN, = A átv MacBook Air
Oxygen gas can be prepared by heating potassium chlorate according to the following equation: 2KC103 (8) 2KCl(s) + 302(g) The product gas, O2, is collected over water at a temperature of 20 °C and a pressure of 757.0 mm Hg. If the wet O₂ gas formed occupies a volume of 5.22 L, the number of moles of KCIO, reacted was 5.3 mol. The vapor pressure of water is 17.5 mm Hg at 20 °C.
Sodium and potassium elements react with water to form hydrogen gas with hydroxide compound. a) Write the reaction equation. b) When 3,196 g of sodium-potassium alloy reacted with excess water, 1,23 liters of hydrogen gas was released at 27 °C and 1 atm. What is the amount of sodium and potassium in the alloy?(Na: 23 g / mol, O: 16 g / mol, H: 1 g / mol, R: 0,082 L.atm / mol.K)
consider an experiment where 4.55mL of an unknown H2O2(aq) solution reacted with the yeast at 19.1 C to produce 98.10ml of gas. what is the partial pressure of O2 (in atm) in the collected gas? 1.0126 atm O2 (this is the correct answer. Can you please show me how to get this calculation) How many moles of O2 were produced by the reaction? 0.004142 mol O2 is the answer.
For many purposes we can treat butane (C,H10) : as an ideal gas at temperatures above its boiling point of – 1. °C. Suppose the pressure on a 43.0 g sample of butane gas at 14.0°C is reduced to one-third its initial value. Oyes Is it possible to change the temperature of the butane at the same time such that the volume of the gas doesn't change? к10 no If you answered yes, calculate the new temperature of the gas. Round your answer to the nearest °C.
11. A sample of gas isolated from unrefined petroleum contains 90.0% CH₁, 8.9% C₂H, and 1.1% C,H, at a total pressure of 3.34 atm. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.) to exerst 30 zalom yu
11. (a) In a 20.0 L steel container, we have only 77.7 g of CO2(g), 66.6 g of N2(g), and O2(g). The temperature is 25.0 ◦C and the total pressure is 8.88 atm. What mass of O2(g) do we have, and what is its partial pressure? The molar masses of C, N, and O are 12.01, 14.01, and 16.00 g/mol. (b) The density of a sample of pure CH4(g) at a constant pressure of 1.00 atm is 0.666 g/L. What is the average speed, or root mean square speed, of the CH4(g) molecules in this sample? The molar masses of C and H are 12.01 and 1.01 g/mol.
PV=nRT R=0.0821 atm•L/mol•K °C + 273.15 = K 1 atm = 760 mmHg Many metals produce hydrogen gas when dropped in water. For example: Ca (s) +2 H20 (1) → Ca(OH)2 (aq) + H2(g) How much hydrogen gas (in liters) would be produced from dropping 5.0 grams of Calcium into an excess of water, at 25°C and 755 mmHg?

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