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What is the equilibrium constant for the following reaction CO(g) + 2 H2(g) ? CH3OH(l); [CO] = 0.530 M and [H2] = 0.824 M?
What mass (in grams) of CH4 is contained in a 555 mL volume at a pressure of 760.0 torr, and at a temperature of 400.0 K?
Nitrogen and oxygen do not react appreciably at room temperature, as illustrated by our atmosphere. But at high temperatures, the reaction below can proceed to a measurable extent.
A flask contains 0.250 of liquid bromine, . Determine the number of bromine molecules present in the flask.
commercial concentrated aqueous ammonia is a solution of 28.0%, by mass, ammonia, NH3, (molar mass=17.0 g/mol) in water. the density pf the solution is .900g/mL.
Using curved arrows to show electron movement and bond formation write a reaction mechanism for the acid catalyzed reaction
A reaction of one liter of chlorine gas with 3 liters of fluorine gas yields 2 liters of a gaseous product. All gas volumes are at the same temperature and pressure. What is the formula of the gaseous product?
Further recylcing reactions that would take the products back to some of the monomers. What reactions to use? What would you get as products
the idea of using the pressure at the bottom of the naoh tank to drive the flow of NAOH to where it will join the HCL
When o-phthaladehyde is treated with base, o-(hydroxymethyl)benzoic acid is formed. Show the mechanism of this reaction.
Calculate the pH and pOH of a solution of HI made by dissolving 3 x 10 ^-5 moles of HI (a strong acid) in 570 mL of water.
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.
Concentrated acids and bases may fall outside this range. Calculate the pH of hydrochloric acid, if the solution is sold as 37 % by weight (37 g HCl / 100 g solution) with a density of 1.18 g/mL.
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