Ethylene (CH₂CH₂) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 100 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 (CH₂CH3) 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 35.0 L reaction tank with 35.0 atm of ethane gas and raises the temperature to 400. °C. He believes K = 0.20 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.

When 145 mL of 0.212 M NaCl(aq) and 145 mL of 0.212 M AgNO3(aq), both at 21.1°C, are mixed in a coffee cup calorimeter, the temperature of the mixture increases to 23.7°C as solid AgCl forms. NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNO3(aq) This precipitation reaction produces 3.14 ✕ 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.

In a coffee-cup calorimeter, 110.0 mL of 1.2 M NaOH and 110.0 mL of 1.2 M HCl are mixed. Both solutions were originally at 22.5°C. After the reaction, the final temperature is 30.5°C. Assuming that all the solutions have a density of 1.0 g/cm³ and a specific heat capacity of 4.18 J/°C.g, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter. AH = 0.182 kJ/mol

Hydrocarbons are compounds that contain only C and H atoms. When a hydrocarbon reacts with O2, CO2 and H2O are formed. Write a balanced equation for the combustion of the following hydrocarbon, a high-octane component of gasoline. Do not include states of matter in your answer. C6H6 (benzene)

A sample of 2.30 g of potato chips was burned in a calorimeter. The calorimeter was calibrated to have a heat capacity of 6.94 kcal/°C. The heat released caused the temperature of the calorimeter to increase 1.75°C. Calculate the food caloric content of the potato chips in nutritional calories per gram to three significant figures. Recall that 1 nutritional calorie (Cal) = 1 kcal.

The copper mineral chalcocite, Cu2S, can be converted to copper simply by heating in air: Cu,S(s) + 0,(g) → 2Cu(s) + SO, (g)

A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with  22.4 mL  of  6.45 M  hydrochloric acid. The temperature of the mixture rises  17.2 ° C.  The density of the resulting solution is 1.00  g   mL  and has a specific heat capacity of 4.184  J   g  ·   ° C . The heat capacity of the calorimeter is 16.97  J   ° C .  Part 1:   (a) Identify the limiting reagent for the reaction.         Part 2:   (b) Calculate the heat of reaction (in J).    qrxn =      ×  10    JEnter your answer in scientific notation.   Part 3 out of 3   (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization =  ____ kj/mol

Measurements show that the enthalpy of a mixture of gaseous reactants increases by 214. kJ during a certain chemical reaction, which is carried out at a constant pressure. Furthermore, by carefully monitoring the volume change it is determined that 62. kJ of work is done on the mixture during the reaction. Calculate the change in energy of the gas mixture during the reaction. Round your answer to 3 significant digits. Is the reaction exothermic or endothermic? 0 kJ exothermic endothermic x10 X Ś U!! 00

What chemical equation corresponds to the enthalpy of formation of OF2(g)?

The specific heat of water is 4.18 J/g⋅∘CJ/g⋅∘C. Calculate the molar heat capacity of water. Express your answer numerically, in joules per mole Celsius, to three significant figures.