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Ethyl chloride vapor decomposes by the first-order reaction C2H5Cl --> C2H4 + HCl The activation energy is 249 kJ/mol and the frequency factor is 1.6 X 10^14 s^-1 The rate constant at 730 K is 2.4 x 10^-4 s^-1. 1) Find the fraction of the ethyl chloride that decomposes in 20 minutes at this temperature. ([C2H5Cl]initial - [C2H5Cl]at 1200 sec) / [C2H5Cl]initial =? 2)Find the temperature at which the rate of the reaction would be twice as fast.
0.0010 mg of H, 0.0116 mg of C, and 0.0310 mg of O. It was also determined that the unknown compound had a molecular weight of 90.0 g/mol.
Determine the partial pressure and total pressure of the gases and Find the partial pressure of carbon dioxide in a gas mixture
A mixture consists of 323 mg of methane, 165 mg of argon, and 223 mg of nitrogen. The partial pressure of nitrogen at 275 k is 19 kPa.
what is happening when Nh4Cl is added to NH3 (a basic solution)? what is happening when HCl is added to NH3? how are these example
If 5.68 g of Cu was added to 3.18 g of S8, How much copper (I) sulfide would be produced?
Draw the structure of Caffeine. Skeletal form only. Locate 2 bonds in the molecule that are obviously polar covalent.
An aqueous solution of ethanol, C2H5OH, is 19.00% ethanol by mass and has a density of 0.9700 g mL-1. Calculate the molarity of the ethanol solution.
An aqueous solution of unoxygenated hemoglobin containing 5 g of protein (M= 64000 g/mol) in the 100cm3 of solution is placed in an insulated vessel.
A 21.496 g sample of magnesium is burned in air to form magnesium oxide and magnesium nitride. when the products are treated with water, 2.813 g of gaseous ammonia are generated.
What is the density of hydrogen gas at 23.0^C and a pressure of 1640 psi?
Calculate what quantity of potassium chlorate that has molecular weight of 122.5 needed to form 33.6 litres of oxygen? Express your answer in grams and assume that temperature and pressue will be in normal condition?
At a certain temperature and pressure 1.4 L of N2 reacts with 2.1 L of O2. If all the N2 and O2 are consumed, what volume of N2O3, at the same temperature and pressure, will be produced?
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