LABORATORY SIMULATION Water Vapor Pressure Table Gases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas, the vapor pressure of the water at that temperature must be subtracted from the total pressure. 1) Consider the following reaction: Mg(s) +2 HC1(ag) → MgCl2(aq) + H2(9) The total pressure of gas collected over water is 725.0 mmHg and the temperature is 21.0°C What is the pressure of hydrogen gas formed in mmHg? Pressure = mmHg

LABORATORY SIMULATION Water Vapor Pressure Table Gases produced by a chemical reaction can easily be collected over water. To determine the pressure of the dry gas, the vapor pressure of the water at that temperature must be subtracted from the total pressure. 1) Consider the following reaction: Mg(s) +2 HC1(ag) → MgCl2(aq) + H2(9) The total pressure of gas collected over water is 725.0 mmHg and the temperature is 21.0°C What is the pressure of hydrogen gas formed in mmHg? Pressure = mmHg

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

Chapter5: Gases

Section: Chapter Questions

Problem 129E

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The toy rockets were engineered so well that now you have dreams of creating a real life replica that can carry people to the space station. Aspirations of becoming rich and famous overcome your thoughts. You know that when this compound (Ammonium perchlorate) is heated at 200 C, it breaks down to a variety of gasses, including N2(g), Cl2(g), O2(g), and H2O(g). You know that the rocket will fly due to the sudden appearance of hot gaseous products in a small initial volume that will result from the rapid increase in the pressure and temperature. What total pressure of gas would be able to be produced at 800 C by igniting 7.0X10^5 kg of NH4ClO4 and allowing it to expand to a volume of 6.4X10^6 L? (ideal gas behavior)
Nitroglycerine ( C3H5N3O9) is a very strong explosive that degrades over time and is too shock sensitive to transport safely. Dynamite is made by combining nitroglycerine with stabilizers and adsorbents, which makes it much safer to use. The explosion of nitroglycerin can be represented by: 4C3H5N3O9(l)→6N2(g)+12CO(g)+10H2O(g)+7O2(g) A stick of 40% dynamite is about 20 cm long and about 3 cm in diameter and weighs 203 grams. It is 40.0% nitroglycerine by mass. What is the total number of moles of gas produced when a stick of 40% dynamite explodes?
A student dissolves 10.3g of ammonium nitrate NH4NO3 in 300.g of water in a well-insulated open cup. He then observes the temperature of the water fall from 22.0°C to 19.3°C over the course of 3.1 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NH4NO3s -> NH+4aq + NO−3aq You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded to the correct number of significant digits. Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. Calculate the reaction enthalpy ΔHrxn per mole of NH4NO3.
Hydrogen peroxide (H2O2) decomposes in the presence of a catalyst to form water and oxygen. The catalyst is added to 5.00 mL of a hydrogen peroxide solution at 25.0 °C, and 49.5 mL of gas is collected over water at a total pressure of 763.8 mmHg.a. Write and balance the chemical reaction (note: catalysts do not appear in balanced chemical equations).b. Look up the vapor pressure of water under these conditions.c. What is the partial pressure of oxygen collected over the water?d. How many moles of oxygen are collected?
Hydrogen peroxide (H2O2) decomposes in the presence of a catalyst to form water and oxygen. The catalyst is added to 5.00 mL of a hydrogen peroxide solution at 25.0 °C, and 49.5 mL of gas is collected over water at a total pressure of 763.8 mmHg.a. Write and balance the chemical reaction. (Note: catalysts do not appear in balanced chemical equations.)b. Look up the vapor pressure of water under these conditions.c. What is the partial pressure of oxygen collected over the water?d. How many moles of oxygen are collected? e. How many grams of hydrogen peroxide were in the original sample?f. What is the concentration (in mol>L) of the hydrogen peroxide solution?g. Which part of this process is conceptually most difficult for your group?
Hw.24.
there is a set of absorbance data that you have obtained while doing an experiment studying the diffusion of potassium permanganate into solutions of water. This diffusion experiment was conducted at three temperatures. Calculate the diffusion rates for each of these temperature conditions. Write your answer in standard notation and use 3 digits past the decimal Diffusion Rate 4°C = __________________ Diffusion Rate 22°C = _________________ Diffusion Rate 37°C = _________________ To show how you calculated the diffusion rates for these temperature - What absorbance values did you choose to calculate the slope for the 37°C condition? __________________ and ________________________ Time (min) 4°C 22°C 37°C 0 0.024 0.108 0.081 5 0.048 0.144 0.221 10 0.069 0.196 0.321 15 0.088 0.224 0.424 20 0.086 0.234 0.580 25 0.089 0.248 0.683
A chemical engineer must calculate the maximum safe operating temperature of a high-pressure gas reaction vessel. the vessel is stainless steal cylinder that measures 40.0 cm wide and 48.0 cm high. the maximum safe pressure inside the vessel has been measured to be 3.60 MPa. For a certain reaction the vessel may contain up to 1.13kg of carbon monoxide gas. Calculate the maximum safe operating temperature the engineer should recommend for this reaction. write your answer in degrees celsius. Round your answer to 3 significant digits.
A sample of magnesium metal reacts completely with an excess of hydrocholoric: Mg(s) + 2 HCl(aq) -- > MgCl2(aq) + H2(g) The hydrogen gas produced is collected over water at 28.0 °C. The volume of the gas is 18 L, and the total pressure in the gas collection vessel is 1.06 atm. Calculate the mass of magnesium metal that reacted in grams. (Vapor pressure of water at 28.0 °C = 28.2 mmHg) Just give the number. The assumption is the value is in grams.
Alka-seltzer is a tablet that people take to control acid indigestion. When it is added to water, Alka-seltzer produces carbon dioxide gas. This gas can produce pressure, causing the top to pop off a film cannister in a specific period of time. Your investigation involves determining how the temperature of water will affect the rate at which carbon dioxide gas forms. The materials that are available to you are: film canister with top, thermometer, water, kettle, ice, Alka-Seltzer tablets, timer a. Hypothesize how temperature will affect the rate at which carbon dioxide forms. (1:1) Give specific reasons for your answer (A:3) b. Based upon the materials listed above, design an experiment to fairly test your hypothesis. Ensure you number your steps. (1:2, C:2) From your experiment, you collect the following data: Temperature Time for top to pop off cannister (s) Cold 60 s Hot 20 s Warm 40 s Table 1: Time it took for top to pop off film canister after Alka-seltzer has been added to water.…
The temperature is 21 degrees Celsius, the temperature of Kelvin is 294.15 Kelvin, the barometric pressure is 751mm Hg, calculate the vapor pressure of water.
Carbon has three allotropes: graphite, diamond, and a metallic form called solid III. Graphite is the stable form of 298 K and 1 atm pressure and at temperatures less than 1440 K. Increasing the pressure on the graphite turns graphite into diamond and then the diamond solid It causes it to transform into III. When applied to graphite at 298 K, graphite to diamond Calculate the pressure that causes the conversion. H298K, (graphite) - H298K, (graphite) = -1900J S298K, (graphite) = 5.73 J / K S298K, (diamond) = 2.43 J / K ,Density of graphite = 2.22 g / cm3 Density of diamond = 3.515 g / cm3

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