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The standard free energy change for the reaction of nitrogen gas with hydrogen gas to produce ammonia is -32.9 kJ. Calculate the equilibrium constant for this reaction at 25°C.
Determine what is the observed rate for the given reaction - empirically determined rate
The rate would decrease because the bromide ion is a weaker base than the iodide ion. C) The potential change cannot be predicted.
At a certain temperature and pressure 2.8 L of N2 reacts with 4.2 L of O2. If all the N2 and O2 are consumed, what volume of N2O3, at the same temperature and pressure, will be produced?
Design a synthesis of 4-(carboxymethyl)-nitrobenzoic acid starting with benzene and any other necessary reagents
If you wish to obtain 10.0 grams of copper metal from copper(ii) sulfide, what mass of copper(ii) sulfide must you use
A total of 5 moles of gas react together to produce 4 moles of gas. They are at equilibrium and the process is exothermic. It may be given as follows
The mass percent of a three component gas sample is 58.0% C2H4O2, 14.6% NH3 and 27.4% CH2O. Calculate the partial pressure (atm) of CH2O if the total pressure of the sample is 0.340 atm.
Write balanced net ionic equations for the reactions that occur when water solutions of the following are mixed. Show molecular, ionic, and net ionic formulas.
Which of the following has the smallest mass? a. 3.50 x 1023 molecules of I2
170 ml of an hcl solution with ph of 2.30 is added to 200 ml of an hno3 solution. the resulting ph is 1.40. what was
A 31.3g wafer of pure gold initially at 69.3^\circ C is submerged into 64.1g of water at 27.7^\circ C in an insulated container. What is the final temperature of both substances at thermal equilibrium
a mixture containing 235 mg of helium and 325 mg of neon has a total pressure of 453 torr. what is the partial pressure of helium in the mixture?
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