cocktail assignment (1) (1)

10 Ethylene (CH, CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 x 10" kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH, CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 29.0 atm of ethane gas and raises the temperature to 500. °C. He believes K =0.30 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K, and the mass percent of ethylene you calculate may not be what he actually observes. % x10

10 Ethylene (CH,CH,) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10º kg of polyethylene are made from ethylene each year, for use in everything from household plumbing to artificial joints. Natural sources of ethylene are entirely inadequate to meet world demand, so ethane (CH,CH,) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. Suppose an engineer studying ethane cracking fills a 60.0 L reaction tank with 22.0 atm of ethane gas and raises the temperature to 500. °C. She believes K =0.050 at this temperature. Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Note for advanced students: the engineer may be mistaken about the correct value of K , and the mass percent of ethylene you calculate may not be what she actually observes. %

16 The odor of fish is due primarily to amines, especially methylamine (CH3NH₂). Fish is often served with a wedge of lemon, which contains citric acid. The methylamine reacts with the citric acid to form an odorless product, methylammonium citrate, thereby making less-than- fresh fish more appetizing. K₁ for CH3NH₂ = 4.407 × 10-4 CH₂NH₂ (aq) + H₂O(1)⇒ CH₂NH3(aq) + OH(aq) A. B. What is the pH of a solution that is 0.7625 M in methylamine at 25.0 °C? pH = Please provider your answer below. t Check answer → A (0) Check answer What is the pH of a solution that is 7.007×104 M in methylamine? pH = Please provider your answer below. (0

In one sentence explain what's wrong with this equation, and rewrite it so that the coefficients are correct.  C3H6(g)+4.5 O2(g)->3CO2(g)+3H2O(g)

What is the percent by mass of 25 g of sodium chloride dissolved in 100 g of water? What is the percent by mass of 90 g of KNO3 dissolved in 400 g of solution? What is the percent by mass of NaHCO3 in a solution containing 20 g NaHCO3 dissolved in 600 g water? You have 150 g of a bleach solution.  The percent by mass of the solute sodium hypochlorite (NaClO) is 3.62%.  How many grams of NaClO are in the solution?

Which of the following is a combustion reaction? O 2CO(g) + O₂(g) - → 2CO₂(g) O H₂CO3(aq) →→→ H₂O(1) + CO₂(g) 2 C8H18(1) + 25 O₂(g) 16 CO₂(g) + 18H₂O(g) Pb(NO3)2(aq) + 2Kl(aq) →→→ 2KNO3(aq) + Pbl2(s) 6 Na(s) + 2 H3PO4(aq) → 2 Na3PO4(aq) + 3H₂(g)

The combustion of gasoline produces carbon dioxide and water. Assume gasoline to be pure octane (C8H18) and calculate how many kilograms of carbon dioxide are added to the atmosphere per 7.8kg of octane burned.

Example: A reaction mixture for the combustion of octane contains 5.0 moles of octane and 50. moles of 02. The balanced equation for the combustion of octane is: 2 C8H18 () + 25 O2 (g) ->> 16 CO2 (g) + 18 H₂O (g) What is the theoretical yield of water produced by this reaction?

Sulfur trioxide dissolves in water to make sulfuric acid, H2SO4. Write a balanced chemical equation and determine the mass of sulfuric acid that can be produced from the reaction of 18.0mL of water (d=00g/mL) and 8.6g of SO3?  Yeast converts glucose (C6H12O6) into ethanol (d=789g/mL) in a process called fermentation. An equation for the reaction can be written as follows: C6H12O6(aq)->C2H5OH(1)+CO2(g) Balance the equation.  If 100.0g of glucose yields 50.0mL of ethanol, what is the percent yield for the reaction?

An organic compound found in many kinds of fruit (apples, bananas, melons, cherries, and strawberries). It is added as an artificial flavoring to some foods and drinks to create sweet, fruity flavors. When combustion analysis was carried out on a 2.50g sample of this ester produces 6.10g of CO2 and 2.50g of H2O. If the molar mass of this compound is 144.21g, what is the molecular formula of this compound?

A certain mixture of gasoline obtained from a petroleum refinery plant was found to contain only isooctane (C8H18; FM = 114.22), methyl tert-butyl ether (C5H12O; FM = 88.15), and tetraethyl lead (C8H20Pb; FM = 323.4), a gasoline preservative. Upon complete combustion of 0.4582 g sample, it was found out that the mass of the CO2 (FM = 44.01) absorbent increases by 1.0702 g, while the mass of residue PbO (FM = 223.2) was determined to be 0.0964 g. From this data, calculate the following: a. % (w/w) C8H18b. % (w/w) C5H12Oc. % (w/w) C8H20Pbd. % (w/w) Pb (FM = 207.2) Answer Letter D only

A certain mixture of gasoline obtained from a petroleum refinery plant was found to contain only isooctane (C8H18; FM = 114.22), methyl tert-butyl ether (C5H12O; FM = 88.15), and tetraethyl lead (C8H20Pb; FM = 323.4), a gasoline preservative. Upon complete combustion of 0.4582 g sample, it was found out that the mass of the CO2 (FM = 44.01) absorbent increases by 1.0702 g, while the mass of residue PbO (FM = 223.2) was determined to be 0.0964 g. From this data, calculate the following: a. % (w/w) C8H18b. % (w/w) C5H12Oc. % (w/w) C8H20Pbd. % (w/w) Pb (FM = 207.2)   Answer a to c only

Suppose you are hired by the Environmental Protection Agency as an engineer to measure sulfur dioxide (SO2) emissions in a small industrial power plant. And suppose you analyze a gas sample and get the following composition: 75.66% N2, 10.24% CO2, 8.27% H2O, 5.75% O2, and 0.0825% SO2. You show these figures to the factory clerk the next day, and he insists that this analysis is erroneous and states that the fuel is natural gas, contains methane and ethane and does not contain sulfur. You ask if another fuel is used, and sometimes they say they use fuel as fuel, but at the time of analysis they say that this fuel is not used. However, your measurements show that the enterprise is using fuel at the time of measurement, and the responsible person accepts this later and accepts that they have made mistakes.a) Calculate the molar ratio of carbon / hydrogen in the fuel and use the result to prove that the fuel cannot be natural gas.b) Assuming that C, H and S are the elements present in the…

Hydrogen is manufactured on an industrial scale by this sequence of reactions: CH4 (g) + H₂O(g) = CO (g) + 3 H₂ (g) K2 CO(g) + H₂O(g) = CO₂ (g) + H₂ (g) The net reaction is: K CH4 (g) + 2 H₂O(g) = CO₂ (g) + 4H₂ (g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K₁ and K₂. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K= 00 ロ・ロ ? K₁

in a pure sample of blue vitriol, there is a Cu content of 25.45% what is the new percentage of Cu in oven-dried blue vitriol?

Vitamin C, ascorbic acid, is an essential nutrient that helps the immune system fight off diseases. One way to consume vitamin C is to eat citrus, like oranges. Ascorbic acid reacts with sodium hydroxide according to the following reaction: HC6H7O6(aq)+NaOH(aq) = NaC6H7O6(aq)+H2O(l) The average orange produces 125.0 mL of juice. A 125.0 mL sample of orange juice required 34.0 mL of 0.0100 M NaOH to complete the reaction. a. What is the concentration of ascorbic acid in the orange juice? b. An adult should consume approximately 90.0 mg of vitamin C a day. How many milliliters of orange juice should someone drink to reach the recommended amount of vitamin C?

Write a chemical equation for the combustion of 1 mol of pentane gas, C5H12(g), to form Carbon dioxide gas and water.

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?

6. Nitric acid, HNO3, is a strong acid in aqueous solutions. It is sold commercially as a concentrated solution with a density of 1.38 kg.L' and containing 62% mass of HNO3. We introduce 10.0 mL of this solution in a 250.00 mL volumetric flask which is then filled to the mark with distilled water. This solution is called S. S is then diluted 100 times to afford solution S'. a. What is the definition of a strong acid? b. What is the concentration of solution S? с. What is the pH of solution S?

Nicotinamide is an important vitamin for metabolism and is soluble in water. A deficiency of this vitamin causes a disease called pellagra. Nicotinamide contains 59.0% C, 5.0% H, 22.9% N, 13.1% O by mass. With the addition of 3.88 g of nicotinamide 30.0 mL of nitrobenzene, C6H5NO2 (d = 1,204 g/mL), the freezing point drops from 5.7 °c to -1.4 °C. What is the molecular weight and formula of this compound (Kd = 8.1 °C/m for nitrobenzene, C: 12,01 g/mol, H: 1,01 g/mol, N: 14,01 g/mol and O: 16,00 g/mol)?