Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2H2, and oxygen gas, O2 to produce the following combustion reaction: 2 C2H2 (g) + 5 O2 (g) →4 CO2 (g) + 2 H20 (g) Imagine that you have a 5.6 L gas tank and a 2.3 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 113 atm, to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer numerically, in terms of atm to 0 decimal places.

Acetylene torches are used for welding. These torches use a mixture of acetylene gas, C2H2, and oxygen gas, O2 to produce the following combustion reaction: 2 C2H2 (g) + 5 O2 (g) →4 CO2 (g) + 2 H20 (g) Imagine that you have a 5.6 L gas tank and a 2.3 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 113 atm, to what pressure should you fill the acetylene tank to ensure that you run out of each gas at the same time? Assume ideal behavior for all gases. Express your answer numerically, in terms of atm to 0 decimal places.

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

The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2Al(OH)3(s) + Al2O3(s) -> 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s) + 3C(s) + 4Al(s) -> 3CO2(g) Suppose the yield of the first step is 74.% and the yield of the second step is 76.% . Calculate the mass of aluminum hydroxide required to make 4.0kg of aluminum. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits.
Consider the following equation for the combustion of acetone (C3H6O), the main ingredient in nail polish remover. C3H6O(l)+4O2(g)→3CO2(g)+3H2O(g) ΔHrxn=−1790kJ if a bottle of nail polish remover contains 161 g of acetone, how much heat would be released by its complete combustion?
* Question Completion Status: A Moving to another question will save this response. Question 26 SHOW WORK Given the following reaction: CaC 2(s) + 2H 20 - C2H 2(g) + Ca(OH) 2(aq) Assume that you place 1.85 g of calcium carbide in excess water and collect the acetylene gas over water. Calculate the maximum amount of gas that should be produced in grams round answer to 3 decimal places omit trailing zeroes The actual volume of acetylene and water vapor collected is 810 ml at 30.5°C with a pressure of 557.524 mmHg. Calculate the actual amount of gas collected(in grams) round answer to 3 decimal places omit trailing zeroes The vapor pressure of water at 30.5°C is 32.35 mmHg. Calculate the percent yield of acetylene. round answer to 2 decimal places omit trailing zeros A Moving to another question will save this response.
When 135 mL of 0.204 M NaCl(aq) and 135 mL of 0.204 M AgNO3(aq), both at 21.5°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 24.0°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 2.81 ✕ 103 J of heat, assuming no heat is absorbed by the calorimeter, no heat is exchanged between the calorimeter and its surroundings, and that the specific heat and density of the solutions are the same as those for water (4.18 J/g·°C, and 0.997 g/mL, respectively). Using this data, calculate ΔH in kJ/mol of AgNO3(aq) for the given reaction. ______________ kJ/mol
6
Balance this unbalanced equation by entering only whole numbers into the blank. If the molar coefficient is 1, enter "1" (do not leave it blank: CaHg + O2 → CO2 + H20
6) A block of rhenium metal (specific heat =0.0329 cal/ gC) is heated to 88.2C and then dropped into 100.0 g of water initially at 26.4 C. The final temperature of the mixture is 32.4C. What was the mass of the block of rhenium?
50 g of solid sodium hydroxide is dissolved in 175 mL of water. Using a coffee-cup calorimeter, the temperature change of the water is measured to be -2.1°C. Which equation best describes this system? NaOH(s)→NaOH(aq) + kJ NaOH(s)+ kJ →NaOH(aq) NaOH(s)→NaOH(l) + kJ NaOH(aq)→NaOH(s) + kJ NaOH(aq)+ kJ →NaOH(s) NaOH(l)+ kJ → NaOH(s) What is the definition of the temperature of a substance? the speed of the slowest particles in the substance, subtracted from the speed of the fastest particles. the heat capacity of the substance times its mass a measure of the average kinetic energy of a system the total heat content of a substance the speed of the fastest particles in the substance Which statement describes an endothermic reaction? The surroundings warm up. The system releases energy. The potential energy of the products is less…
A 6.79 g sample of NH, gas and a 6.79 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C. < EFeedback You have not correctly determined the mass of NH,Cl formed. Identify the limiting reagent. Convert the given mass of the limiting reagent to the mass of NH,Cl using the NH; mole ratio from the balanced chemical HCI equation and the molar masses for both NH,CI the limiting reagent and the NH,Cl as conversion factors. How many grams of NH,Cl will be formed by this reaction? 0.273 mass: Incorrect What is the pressure in atmospheres of the gas remaining in the flask? Ignore the volume of solid NH,Cl produced by the reaction. P = 3.42
True or False: The test tube in which a chemical reaction is taking place feels warmer to the touch. The reaction is endothermic.
Consider the following chemical reaction which produces nitric oxide from its constituent elements: N2 (g) + O2(g) → 2 NO (g) AH = 182.6 kJ/mol If nitrogen and oxygen were mixed and allowed to react under constant pressure conditions, which of the following statements must be true? Select as many answers as applicable however points will be deducted for incorrect guesses. ΔΗ = q This is an endothermic reaction The temperature of the surroundings would decrease The temperature of the surroundings would increase AH = AU
When NO(g) reacts with O2 (g) according to the following reaction, 57.1 kJ of energy are evolved for each mole of NO(g) that reacts. Complete the following thermochemical equation. 2NO(g) + O₂(g) → 2NO2(g) AH = ? ΔΗ = kJ