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At some temperature,a 100-L reaction vessel contains a mixture that is initially 1.00 mol CO and 2.00 mol H2. The vessel also contains a catalyst so that the following equilibrium is attained:
CO(g)+ 2H2(g) <---- ----> CH3OH(g)
At equilibrium, the mixture contains 0.100 mol CH3OH (methanol). In a alter experiment in the same vessel, you start with 1.00 mol CH3OH. How much methanol is there at equilibrium? explain
Calculate the theoretical yield of C2H5Cl when 138 g of C2H6 reacts with 244 g of Cl2, assuming that C2H6 and Cl2 react only to form C2H5Cl and HCl.
why is it important to immediately cover the Mg ribbon with the other slab of dry ice once it starts burning?
What will be the final temperature of a 15.0g sample of water that is heated with the addition of 4.2kJ at 18 0C
Concentrated HCl is 36.5% HCl by mass and has a density of 1.18 g/mL.What is the molality?What is the molarity?
What is the partial pressure of hydrogen and nitrogen when the gas mixture is composed of 8.00 g hydrogen and 56 grams nitrogen.
the lead in lead pencils is actually almost pure carbon, and the mass of a period mark made by a lead pencil is about 0.0001g. How many carbon atoms are in the period.
Empirical and Molecular Formulae, The analysis of an organic compound produces the following elemental analysis: % C is 59.999% and % H is 4.476%.
Calculate the volume of glacial acetic acid needed to make 1L of the buffer. Glacial acetic acid is 99.5% acetic acid
A catalyst decreases the activation energy of a particular exothermic reaction by 59 kJ/mol, to 51 kJ/mol. Assuming that the mechanism has only one step, and that the products are 94 kJ lower in energy than the reactants
Compare the amount of cooling experienced by an individual who drinks 400mL of water (0 degrees C) with the amount of cooling experienced by an individual who sweats out 400 mL of water at 37 degrees Celsius. Assume all sweat evaporates.
Determine the rat of consumption of O2 if the initial concentration of NH3 was 0.6719 M and decreased to 0.5827 M after 0.3883 hours
CS2(l) + 3O2(g) -> CO2(g) + 2SO2(g) What volume of O2 is required to react with excess CS2 to produce 4.0 L of CO2? Assume all gases are measured at 0oC and 1 atm.
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