Ethylene (CH₂CH₂) is the starting point for a wide array of industrial chemical syntheses. For example, worldwide about 8.0 × 10¹0 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 (CH3 CH3) from natural gas is "cracked" in refineries at high temperature in a kinetically complex reaction that produces ethylene gas and hydrogen gas. 圖 Suppose an engineer studying ethane cracking fills a 50.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 600. °C. She believes Kp = 0.70 at this temperature. dlo Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits. Ar Note for advanced students: the engineer may be mistaken about the correct value of Kp, and the mass percent of ethylene you calculate may not be what she actually observes. 99 % X 5 ? Explanation Check
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
![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 (CH3CH3) 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 50.0 L reaction tank with 20.0 atm of ethane gas and raises the temperature to 600. °C. She believes
K = 0.70 at this temperature.
р
alo
Calculate the percent by mass of ethylene the engineer expects to find in the equilibrium gas mixture. Round your answer to 2 significant digits.
Ar
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.
%
x10
X Ś
?
Explanation
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this one is asking for kg
![Sulfuric acid is essential to dozens of important industries from steelmaking to plastics and pharmaceuticals. More sulfuric acid is made than any other industrial
chemical, and world production exceeds 2.0 × kg per year.
10¹1
The first step in the synthesis of sulfuric acid is usually burning solid sulfur to make sulfur dioxide gas. Suppose an engineer studying this reaction introduces
2.6 kg of solid sulfur and 6.50 atm of oxygen gas at 700. °C into an evacuated 60.0 L tank. The engineer believes K₂=0.38 for the reaction at this
temperature.
Calculate the mass of solid sulfur she expects to be consumed when the reaction reaches equilibrium. Round your answer to 2 significant digits.
olo
Note for advanced students: the engineer may be mistaken in her belief about the value of K, and the consumption of sulfur you calculate may not be what
she actually observes.
Ar
kg
x10
X Ś
?
Explanation
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This one is a little different, but can u answer it as well
![Nitrogen forms a surprising number of compounds with oxygen. A number of these, often given the collective symbol NOx (for "nitrogen + x oxygens") are
serious contributors to air pollution. They can often be interconverted, sometimes by reaction with oxygen or ozone (03) in the air.
An atmospheric scientist decides to study the reaction between nitrogen trioxide and nitrogen monoxide that produces nitrogen dioxide. He fills a stainless steel
reaction chamber with 1.5 atm of nitrogen trioxide gas and 8.3 atm of nitrogen monoxide gas and raises the temperature considerably. At equilibrium he
measures the mole fraction of nitrogen dioxide to be 0.19.
Calculate the pressure equilibrium constant K for the equilibrium between nitrogen trioxide, nitrogen monoxide, and nitrogen dioxide at the final temperature
р
of the mixture.
olo
Round your answer to 2 significant digits.
Ar
K₁ =
0x₁
P
Ś ?
Explanation
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