a. Sulphur trioxide (SO3) is produced in an industrial scale from sulphur (S) andoxygen (O2). For simplicity, let's assume this is a one-step reaction.How many m³ of air with (O2) = 21 %, T = 18 °C and 325 kPa are required toproduce 58 t of SO3, if you calculate a volume excess for O2 of 23 %?b. Upon reaction of SO3 with water, sulphuric acid is formed. Formulate thereaction equation and calculate which volume of water you would need toconvert all SO3 from a. into sulphuric acid?

Step 1: Calculate the number of moles of O2 needed to produced 58 tons of SO3 using stoichiometric…

Answered: a. Sulphur trioxide (SO3) is produced…

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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Calculate the pressure exerted by 1 mol of an ideal gas in a box that is 0.500 L and 298 K. Have each group member calculate the pressure of 1 mol of the following gases in the same box at the same temperature: He, Ne, H2, CH4, and CO2. Compare group members’ answers as well as all answers with the pressure of an ideal gas. Assuming that the van der Waals equation predictions are accurate, account for why the pressure of each gas is higher or lower than that predicted for an ideal gas.
1. The compressibility factor Z = PV/nRT for O2 at -27.1°C and 537.1 atm is 1.50; at 147.4°C and 95.5 atm, it is 1.02. A certain mass of oxygen occupied a volume of 3.28 L at 147.4°C and 95.5 atm. Calculate the volume occupied by the same quantity of oxygen at -27.1°C and 537.1 atm. 2. The composition of a mixture of gases in percentage by volume is 20.5% nitrogen, 15.7% carbon monoxide, 37.8% water, and the rest sulfur dioxide. Calculate the density of the gaseous mixture at 39.8°C and 1.46 atm in grams/liter. Report your answer to the hundredths position.
c. Calculate the mole fraction of chlorine and its partial pressure in the mixture of gases produced. d. The van der Waals equation applies strictly to pure real gases.P = (nRT/ V-nb) – a(n2/V2) Suppose the gas mixture generated in the decomposition has the following parameters: a= 4.00 atm*L2/mol2 and b = 0.0330 L/mol. Determine the pressure of the gas mixture in part (b) using the van der Waals equation. Why is the result smaller than that in part (b)?
The concentration of gases, polluting or not, is usually expressed in ppm or ppb. Consider an air sample with 320 micrograms/m3 of SO2. What will be the concentration of this sample in ppb if the total air pressure is 1,0 atm and the temperature 27 oC
A 6.00L tank C is filled with 4.09g of cabron monoxide gas and 4.36g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
A quantity of 0.225 g of a metal A molar mass = 27.0 g mol liberated 0.303 L of molecular hydrogen (measured at 17 °C and 741. mmHg) from an excess of hydrochloric acid. Deduce from these data the corresponding equation and write the formulas for an oxide and a sulfate of A. Note: Reference the Fundamental constants and Conversion factors for non-SI units tables for additional information. Part: 0/3 Part 1 of 3 Using the smallest whole-number coefficients, write the balanced equation for the reaction of the metal, A, with hydrochloric acid. Include the phase abbreviations. ☑ → A) + 2HCl(aq) ACI, (e) + H₂(aq) ローロ
8. ) ( delete 8. 9.
Deduce the balanced reaction in which ammonia reacts with nitrogen dioxide to produce molecular nitrogen and water. Using 1000 L of air at 27 degrees C and 1 atm pressure containing 10 ppm of NO2. [Hint: Recall from introductory chemistry that PV=nRT and that a balanced equation indicates the number of moles of the substances that react with each other.]
Can you help me please? If it includes these in the question, can you solve it using significant figures and dimensional analysis?
Hand written solutions are strictly prohibited.
‏You are working in an oil refinery . Where you use hydrocarbon gases like methane ( CH4 ) , ethane ( C2H5 , and propane ( C3Hg ) and prepared a mixture . When measured the pressure at 25 ° C it turns out to be 7.50 am This gas mixture was then also used in a mass spectrophotometer and the following data was obtained Based on this information find the partial pressure of each gas and report respectively as their name .appeared in the question
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