When ozone (O3) is placed in contact with dry, powdered KOH at –15°C, the red-brown solid potassium ozonide (KO3) forms, according to the following balanced equation: 5 O3(g) + 2 KOH(s) → 2 KO3(s) + 5 O2(g) + H,O(s) Calculate the volume of ozone needed (at a pressure of 0.134 atm and – 15°C) to produce 4.69 g KO3.

When ozone (O3) is placed in contact with dry, powdered KOH at –15°C, the red-brown solid potassium ozonide (KO3) forms, according to the following balanced equation: 5 O3(g) + 2 KOH(s) → 2 KO3(s) + 5 O2(g) + H,O(s) Calculate the volume of ozone needed (at a pressure of 0.134 atm and – 15°C) to produce 4.69 g KO3.

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...

See similar textbooks

Similar questions

1) Calculate the volume of 1.62g of Helium gas at 25.670C and 872 mmHg. (R = 0.0821 atm.L/mol.K) 2) Given the following reaction of Ca(s) in HCl(aq): Ca(s) + 2 HCl(aq) --> CaCl2(aq) + H2(g) If 32.7g of calcium solid are placed in this reaction and at the end of the experiment, hydrogen gas is produced at 25.000C and with a pressure of 790. mmHg. Calculate the volume of hydrogen gas produced. 3) An unknown gas with a mass of 1.211g occupies a volume of 677 mL. The temperature is 230C and the air pressure is 0.987 atm. Calculate the molar mass of the gas.
A 10.0 L vessel at 298 K contains O2(g) at a pressure of 740. mmHg. What mass of He(g) would be added to increase the total pressure to 1480. mmHg?
Water can be decomposed by electrolysis to hydrogen gas and oxygen gas. If 2.33 g of water is decomposed to H2(g) and O2(g) and the gases are collected in a 1.00 L flask over water at 25°C (vapor pressure H2O(l) = 23.8 mm Hg), what is the pressure in the flask?
The air bags in automobiles were once inflated by nitrogen gas generated by the rapid decomposition of sodium azide, NaN3. 2 NaN3 (s) → 2 Na (s) + 3 N2 (g) If an air bag has a volume of 50 L and is to be filled with nitrogen gas at a pressure of 1.06 atm and a temperature of 22.8°C, how many moles of NaN3 must decompose? You may assume the N2 behaves as an ideal gas. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter your response to four decimal places. Carmen may add or remove digits from your response, your submission will still be graded correctly if this happens.
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.
A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)
A sample of 3.42 mol of xenon is confined at low pressure in a volume at a temperature of 86 °C. Describe quantitatively the effects of each of the following changes on the pressure, the average kinetic energy per molecule in the gas, and the root-mean-square speed. (a) The temperature is increased to 199 °C (b) The volume is tripled. (c) The amount of xenon is decreased to 1.87 mol Give each answer as a decimal factor of the form: new value factor old value. A factor of 1 means no change. ChangeP KEavgms
What is the density of CO2 at 655 mmHg and 55oC?
Given the reaction: 2 Al (s) + 6 HCI (ag) --> 2 AICI3 (aq) + 3 H2 (g) A strip of aluminum of unknown mass is reacted with excess hydrochloric acid. When the hydrogen gas is collected over water, it is done so at a temperature of 22.0 °C and fills a flask of volume 32.5 mL. The pressure inside the collection tube is 756.1 mmHg and the water vapor pressure at 22.0 °C is 19.83 torr. Determine the mass of the aluminum strip in milligrams (mg).
0.300 mol of O2 gas is held at an a 5.00 L container at 45.0 °C. Determine the following:(a) the volume this gas occupies at ST (in L).(b) the pressure of this gas if the temperature isincreased to 60.0 °C assuming the volume does notchange.(c) the volume of NO2 (in L) expected from complete combustion of the excess N2 in O at STP.Hint: Use answer from (a) as a starting point.
A sample of H2(g) was collected over water in a volume of 12.0 mL at 18 °C under atmospheric pressure of 770. Torr. Partial pressure of water is P(H2O, 18 °C) = 16 Torr. Find the mol’s of H2(g) in the sample
@