Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2 H2, and oxygen gas, O2 to produce the following combustion reaction: 2C2 H2 (g) + 502 (g)→4CO2 (9)+ 2H20(g) You have a 7.00 L gas tank and a 2.50 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 145 atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time?

Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2 H2, and oxygen gas, O2 to produce the following combustion reaction: 2C2 H2 (g) + 502 (g)→4CO2 (9)+ 2H20(g) You have a 7.00 L gas tank and a 2.50 L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 145 atm , to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time?

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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Acrylonitrile is an important building block for synthetic fibers and plastics. Over 1.4 billion kilograms of acrylonitrile are produced in the United States each year. The compound is synthesized from propene (C3H6) in the following reaction: 2C3H6(g) + 2NH3(g) + 30₂(g) →2C3H3N(I) + 6H₂O(g) Determine how many kg of acrylonitrile can be prepared from 1480 kg of propene, 788 kg of ammonia, and 1980 kg of oxygen.
The human body burns glucose (C6H₁2O6) for energy according to this chemical reaction: C6H12O6 +60₂-6CO₂ + 6H₂O The products of the reaction are carbon dioxide (CO₂) and water (H₂O). Interestingly, all of the carbon dioxide and much of the water exits the body through the lungs: on every breath, the average person exhales 500. mL of air, which is typically enriched to 4% CO₂ and 5% water vapor by volume. In short, when a person loses weight by dieting, the weight that is lost actually departs his body as a gas, every time he exhales. Each kilogram of body fat lost requires exhaling about 2.9 kg of carbon dioxide. Calculate how many breaths it takes an average person to "exhale" 1.00 kg of fat. Round your answer to the nearest thousand. You'll need to know that the density of CO₂ is 2.0 kg/m³. 0 ☐ ☐x10 X
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 53.0mL of dioxygen gas are produced by this reaction, at a temperature of 50.0°C and pressure of exactly 1atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N₂(g) + 3H₂(g) 2 NH, (g) In the second step, ammonia and oxygen react to form nitric acid (HNO3) and water: NH₂ (g) + 20₂(g) → HNO3(g) + H₂O (g) Suppose the yield of the first step is 61.% and the yield of the second step is 77.%. Calculate the mass of nitrogen required to make 10.0 kg of nitric acid. Be sure your answer has a unit symbol, if needed, and is rounded to 2 significant digits. 0 Explanation Check. ☐ x10 8 X 09 0.0 S © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |
Copper(II) sulfate, CuSO4, reacts with sodium hydroxide, NaOH, in a double displacement reaction. The products are a precipitate of copper (II) hydroxide, Cu(OH)2, and an aqueous solution of sodium sulfate, Na2SO4. CuSO4(aq) + 2NaOH(aq) → Cu(OH)2(s) + Na2SO4(aq) 50.0 mL of 0.300 mol/L CuSO4 solution are mixed with an equal volume of 0.600 mol/L NaOH. The initial temperature of both solutions is 21.4°C. After mixing the solutions in a calotimeter, the highest temperature reached is 24.6 oC. Determine the change in the enthalpy of the reaction. Then write the thermochemical equation.
A studen wanted to determine the value of R and so used the reaction: Mg(s) + 2 HCl(aq) → H2(g) + MgCl2 (aq) She got a piece of magnesium ribbon and determined its mass as 0.0841 g. She placed the ribbon in a test tube with water and excess HCl and inverted it to allow the H2 gas to bubble to the top of the tube while water was pushed out the bottom. She measured the volume of the gas in the tube as 87.8 mL. She measured the temperature of the water at 20.5ᵒC and the atmospheric pressure in the room was 751 torr. 1- What other piece of information did she have to determine in order to accurately calculate R? 2- What did she calculate for the value of R? 3- What was her % error?
The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 71.0 mL of dioxygen gas are produced by this reaction, at a temperature of 50.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Be sure your answer has the correct number of significant digits.
This equation models how pure silver (Ag) is extracted from ores of AgK(CN)2 (potassium argentocyanide), which is mined from the earth. Zinc is a reactant in the equation, and it is needed in order to extract the silver from the potassium argentocyanide ore. 2AgK(CN)2(aq)+Zn(s)→2Ag⁡(s)+Zn(CN)2(aq)+2KCN(aq) How many atoms of pure zinc (Zn) are needed in the production process to create a pure silver coin of mass 31 grams?
Calcium hydride reacts with water to produce hydrogen gas according to the following reaction: CaH2(s) + 2 H2O(l) ----> 2H2(g) + Ca(OH)2(aq) This reaction is used to generate hydrogen gas to inflate air bags in cars and life rafts on boats and for similar uses where a simple compact means of hydrogen generation is necessary. Assuming complete reaction with water, how many grams of calcium hydride are required to fill a raft to a total pressure of 2.0 atm at 25oC if the volume of the raft is 1,000 L?