14. A student thermally decomposed a 0.160 gram sample of impure potassium chlorate (KCIO3; 122.5 g/mole). Manganese dioxide (MnO2) was used as a catalyst. The student collected 45.00 mL of oxygen gas in a eudiometer over water. Potassium chloride is the other product of the reaction. At the time, the temperature was 22.22 °C and the atmospheric pressure was 771.00 mm Hg. The water level in the eudiometer was 7.00 cm above the water level in the beaker. The vapour pressure of water at this temperature is 18.11 mm Hg. [1 mm Hg 13.6 mm H2O; O2 = 32.00 g/mole; R = 0.082057 L Atm/mol K; PV = nRT; V1PIT2 = V2P2T1; 1 cm 10 mm; K = °C + 273.15] a] Write a balanced equation for the thermal decomposition of potassium chlorate: 2KC10 3 † MnOz -330, +2KCI b] Determine the volume, in mL, of the "dry" oxygen gas at STP conditions c] What is the percent purity of the potassium chlorate sample?

14. A student thermally decomposed a 0.160 gram sample of impure potassium chlorate (KCIO3; 122.5 g/mole). Manganese dioxide (MnO2) was used as a catalyst. The student collected 45.00 mL of oxygen gas in a eudiometer over water. Potassium chloride is the other product of the reaction. At the time, the temperature was 22.22 °C and the atmospheric pressure was 771.00 mm Hg. The water level in the eudiometer was 7.00 cm above the water level in the beaker. The vapour pressure of water at this temperature is 18.11 mm Hg. [1 mm Hg 13.6 mm H2O; O2 = 32.00 g/mole; R = 0.082057 L Atm/mol K; PV = nRT; V1PIT2 = V2P2T1; 1 cm 10 mm; K = °C + 273.15] a] Write a balanced equation for the thermal decomposition of potassium chlorate: 2KC10 3 † MnOz -330, +2KCI b] Determine the volume, in mL, of the "dry" oxygen gas at STP conditions c] What is the percent purity of the potassium chlorate sample?

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

Related questions

Q: Here is the overall reaction in an automobile air bag: 20NAN (s) + 6S1O, (s) + 4KNO,(s) → 32N,(g) +…

Q: This reaction occurs at constant temperature and pressure. The container in which this reaction is…

A: The balanced reaction taking place is given as, => 2 H2 (g) + 1 CO (g) ------> 1 CH4O (g)…

Q: A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas…

Q: In an experiment of 0.609 atm wer

A: As you have posted a question with multiple parts, we will solve the first question for you. To get…

Q: You are heating potassium perchlorate and collecting the oxygen gas from the decomposition over…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: 3 RT speed = V M %3D = 8.314 J/ (mol-K) and M is molar mass in kilograms per mole. Note that a joule…

A: rms speed = (3RT/M)1/2 For F2 molecules, M = 38 g/mol = 38×10-3 Kg/mol So, rms speed= =…

Q: A student decomposed 6.900 g of solid ammonium nitrite (MW = 64.04 g/mol) at a temperature of 30.00…

A: Solid ammonium nitrite undergoes decomposition according to the problem. We are asked to write the…

Q: A 0.0665 g sample of aluminum metal reacts with hydrochloric acid to give 90.5 mL of hydrogen gas at…

A: Stoichiometry relates the amount of reacting with the formed species. As per this concept, the…

Q: The airbags that protect people in car crashes are inflated by the extremely rapid decomposition of…

Q: The reaction vessel containing NOCI(g) is maintained at 27.0 °C until equilibrium has been achieved…

A: The balanced reaction taking place is given as, => 2 NOCl -----> 2 NO + Cl2 Given : Initial…

Q: A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas…

A: Data given: Width of the cylindrical reaction vessel, w = 48.0 cm Height of the cylindrical reaction…

Q: 1. First, 0.9144 grams of the material was placed into an evacuated 0.500 L container. The…

A: “Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: A 2.20 L container at 53.6 °C contains 6.21 g of N2O3(g). The N2⁢O3 gas decomposes completely,…

A: Volume of container V = 2.20 L Temperature T = 53.6 degree C = 53.6 + 273.15 K = 326.75 K Mass of…

Q: Calculate the total volume of gas (at 29 °C and 749 mm Hg) produced by the complete decomposition of…

A: The Balanced Equation:Temperature = 29 oC and Pressure = 749 mm Hg Complete decompostion of 1.36 Kg…

Q: Part 5. Dalton's Law of Partial Pressures A sample of Argon gas is placed in a 5.0L container at…

A: According to the Dalton's law of partial pressures, the total pressure of the gaseous mixture is the…

Q: A Haber process reactor contains 25.0% nitrogen and 75.0% hydrogen for the synthesis of ammonia.…

Q: A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas…

A: First we need to calculate the volume of cylinder. Then we need to calculate the moles of gas from…

Q: What is the experimental molar mass (that is, calculated from the data given and not taken from the…

A: a). Pressure ( P ) = 727.5 torr = ( 727.5 / 760 ) atm = 0.957237 atm Temperature ( T ) = 22.2 °C =…

Q: The generic reaction occurs in a closed container: 2A(g) +B(g) → 2Ce) A reaction mixture initially…

Q: If a small volume of a particular liquid was to react with the oxygen in the atmosphere, which…

A: A system is defined as the part of the universe where we perform our work. The region outside the…

Q: A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas…

A: I Hope its helpfull.thank you.

Q: O number of molecules.

A: Answer: equal volume propane and carbon monoxide at the same temperature and pressure have the…

Q: A 2.53 L container at 74.1 °C contains 6.31 g of N2O3(g). The N2O3 gas decomposes completely,…

Q: A reaction between liquid reactants takes place at -7.0 °C in a sealed, evacuated vessel with a…

A: Given: The mass of CO gas = 13 g The volume of the vessel = 20.0 L Temperature = -7.0 ∘C We have to…

Q: A reaction is carried out using 0.0754 g of magnesium and an excess of HCl(aq), and the H2 gas is…

Q: 5) Consider the reaction below. CO(g) + 2H2(g) → CH;OH(9) 1.5 L of hydrogen gas and 3.5 L of carbon…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

14. A student thermally decomposed a 0.160 gram sample of impure potassium chlorate (KCIO3; 122.5
g/mole). Manganese dioxide (MnO2) was used as a catalyst. The student collected 45.00 ml of oxygen gas
in a eudiometer over water. Potassium chloride is the other product of the reaction. At the time, the
temperature was 22.22 °C and the atmospheric pressure was 771.00 mm Hg. The water level in the
eudiometer was 7.00 cm above the water level in the beaker. The vapour pressure of water at this
temperature is 18.11 mm Hg.
[1 mm Hg = 13.6 mm H2O; 02 = 32.00 g/mole; R = 0.082057 L Atm/mol K;
PV = nRT; V1P1T2 = V2P2T1; 1 cm = 10 mm; K = °C + 273.15]
%3D
a] Write a balanced equation for the thermal decomposition of potassium chlorate:
2KC103 + MnOz ->30, +2KCI
b] Determine the volume, in mL, of the "dry" oxygen gas at STP conditions
c] What is the percent purity of the potassium chlorate sample?

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Trending now

This is a popular solution!

Step by step

Solved in 5 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

An unknown mass of aluminum is added to HCl solution. The aluminum metal is completely dissolved in the solution and generates hydrogen gas. See the balanced equation for the gas evolution reaction: 2 Al(s) + 6 HCl(aq) ---> 2 AlCl3(aq) + 3 H2(g) The following data is collected: Mass of Al sample: unknown g Volume of gas collected 45.38 mL Barometric pressure 754.8 mmHg Temperature 23.5OC Vapor pressure of H2O at 23.5OC 21.65 mmHg Hydrogen gas is collected over water. The reaction proceeds until all the amount of aluminum is consumed in the gas-evolution reaction (aluminum is the limiting reactant). (a) Calculate the mole number of the hydrogen gas generated in the reaction: Convert the volume of the collected gas to L: 45.38 mL = ___________ L Calculate the pressure exerted by H2 gas (= dry hydrogen gas): Pressure of the dry hydrogen gas =…
At 25 °C and 765.6 torr, a sample that is a gaseous compound containing carbon, hydrogen, and oxygen occupies a volume of 0.582 L. A mass of 1.103 g of this sample was burned in a bomb calorimeter, producing 1.294 g of liquid water and 2.108 g of gaseous carbon dioxide. The heat produced from the combustion raised the temperate of the calorimeter from 25 °C to 31.94 °C. a.) What is the percent elemental composition by mass of the unknown sample. b.) Determine the empirical formula of the sample.
HCl(g) can be made by the direct reaction of H2 and Cl2 in the presence of light. 6.00 g of H2 and 1.50 x 102 g Cl2 are mixed in a 5.00 L flask at 28.0 °C. What are the partial pressures of gases after the reaction has completed. Given Information: > Temperature and volume remains constant at 28.0 °C > Wavelength of light needed for the reaction is 340 nm.
The solid rocket propellant for the Space Shuttle (and Tomahawk Missiles) contain ammonium perchlorate, NH,CIO4(s) , and aluminum powder, Als) bound together with polymer (rubber) compound. The reaction that provides the thrust for these engines is given below: 6 NH4CIO4(s) + 10 Al(s) → 4 Al203(s) + 2 AlCl3(s) + 12 H2O(g) + 3 N2(9) ; AHº, rxn ΔΗΡ -289 kJ/mol 0.0 kJ/mol -1675.5 kJ/mol -705.6 kJ/mol -241.8 kJ/mol 0.0 kJ/mol Use the enthalpies of formation (AHº;) to calculate the change in enthalpy, AH® x, for this reaction (~ 6 mols of NH4CIO4(s). AH°, [ Select ] kJ/ 6 mol NH4CIO4(5) rxn
#15
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.
In one demonstration of this reaction, 36.00 mL of H2 are collected over water at 25°C. Atmospheric pressure is 749.0 mmHg. How many grams of H2 are collected? g Hydrogen
8. In one lab this semester, you ran the reaction: KC1O3 (s) → KCl (s) + O2 (g). The directions asked you to add about 1.5 g KC1O3 to a crucible. How many liters of O2 should form at STP?