The research and development unit of Air Liquid company is studying the reaction between two components of natural gas : CH4 (g) + 2 H₂S (g) = CS₂ (g) + 4 H₂ (g) At one point in the experiment, 1.00 mol of CH4, 1.00 mol of CS2, 2.00 mol H₂S and 2.00 mol of H₂ are mixed in 200 mL vessel at 960 °C. At this temperature, K₂ = 0.036 (i) (ii) Predict the direction of reaction to reach anequilibrium. State the name of the principle used to justify the counter effect.

The research and development unit of Air Liquid company is studying the reaction between two components of natural gas : CH4 (g) + 2 H₂S (g) = CS₂ (g) + 4 H₂ (g) At one point in the experiment, 1.00 mol of CH4, 1.00 mol of CS2, 2.00 mol H₂S and 2.00 mol of H₂ are mixed in 200 mL vessel at 960 °C. At this temperature, K₂ = 0.036 (i) (ii) Predict the direction of reaction to reach anequilibrium. State the name of the principle used to justify the counter effect.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 74QAP: Magnesium ribbon reacts with acid to produce hydro- gen gas and magnesium ions. Different masses of...

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Magnesium ribbon reacts with acid to produce hydro- gen gas and magnesium ions. Different masses of magnesium ribbon are added to 10 mL of the acid. The volume of the hydrogen gas obtained is a measure of the number of moles of hydrogen produced by the reaction. Various measurements are given in the table below. (a) Draw a graph of the results by plotting the mass of Mg versus the volume of the hydrogen gas. (b) What is the limiting reactant in experiment 1? (c) What is the limiting reactant in experiment 3? (d) What is the limiting reactant in experiment 6? (e) Which experiment uses stoichiometric amounts of each reactant? (f) What volume of gas would be obtained if 0.300 g of Mg ribbon were used? If 0.010 g were used?
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
Sulfuric acid can be manufactured using the reaction: 2S(s) + 3 O2(g) + 2 H2O(l) -> 2 H2SO4 (aq) if a manufacturing site consumes 65 metric tons (1 metric ton = 1000kg) of sulfur with unlimited access to O2 and H2O, how many metric tons of sulfuric acid may be produced?
Consider the titanium thermite reaction: Ti2O3 (s) + 2 Al (s) -----> Al2O3 (s) + 2Ti (l) You attempt this reaction with 100.0g of Ti2O3 and 100.0g of 100.0g of powdered aluminum(Al). c) Determine the mass of liquid titanium produced by this reaction. d) What is the Percentage Yiled of liquid titanium if we were only able to produce 40.0g of the product?
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A General Chemistry student performed the “Thermochemistry” lab and obtained the following results: C. ΔH for Reaction of HCl(aq) and NaOH(s):Volume of HCl: 0.0550 LVolume of water: 0.0450 LVolume total: 0.1000 LMolarity of HCl: 2.15 MMass of NaOH: 2.150 gΔT for reaction C: 34.2 °C Using NaOH as the limiting reagent, calculate the molarity of the resulting sodium chloride solution. Calculate the total number of calories produced in the reaction. Calculate the ΔH for this reaction.
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C9H8O4 is synthesized by reacting stoichiometric amounts of C7H6O3 and (CH3CO)2O, as shown by the balanced chemical equation in the picture: During the synthesis, 500 grams of salicylic acid was available for use in the experiment. Other information: MW of Salicylic Acid: 138.121 g/mol MW of Acetic Anhydride: 102.09 g/mol Density of Acetic Anhydride: 1/08 g/ml Question: The available Acetic anhydride reagent in the lab is in the liquid form. How many mL of Acetic anhydride is needed to react with the available salicylic acid stoichiometirically?
Photosynthesis is a process that incorporates carbon dioxide and water and yields food in the form of glucose (CGH1206) for the plant with oxygen (02) as the by-product. In a (5) five minute period a tree consumes 600 grams of water and enough carbon dioxide that is in excessive amounts in the atmosphere. Determine the amount of glucose and oxygen that is produced
The hydrated salt, MY3·xH2O, was heated strongly in a crucible to remove all the watermolecules of crystallization.The data are for this experiment are given in the table below.Mass of empty crucible and cover 29.73 gMass of crucible, cover, and hydrated salt 32.72 gMass of crucible, cover, and anhydrous salt 31.52 gMolar mass of anhydrous salt 241.88 g/mol(i) Calculate the % composition by mass of water in the hydrated salt.(ii) Determine the value of x.(iii) M is in Period 4 of the Periodic Table of the Elements.If Y = NO3–, identify the element M.(iv) What is the name of this hydrated salt? ___