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Calculate the number of collisions per second of one hydrogen molecule at 24 °C and 8.00 bar. The diameter of a hydrogen molecule is 270 pm. I am having trouble with the calculations. Is there a specific way to put this in my calculator?
Draw a diagram for this cell and identify the cathode (including the identity of metal), anode (including the identity of metal), direction of electron flow, salt bridge, and ions present in solutions.
The concentration of Mg2+ in seawater is 0.052 M. At what pH will 74% of the Mg2+ be precipitated as the hydroxide salt? [Ksp for Mg(OH)2 = 8.9* 10-12.]
If 18.5 mL of 0.800 M HCl solution are needed to neutralize 5.00 mL of a household ammonia solution, what is the molar concentration of the ammonia.
Draw its lewis structure, with the lone pair electrons, with the formal charges minimized? NO4 3-
Calculate the mass of the sample of silver. Can you please explain how you answered this question so I can understand it on my final?
Trouble understanding the relationship between the Ka and how acidic a chemical is. Is it safe to say that the more acidic a chemical is the higher the Ka value will be
Estimate the temperature you should dope at (°C) if you must have a concentration of 100 P atoms per 10 million Si atoms at a depth of 10 nm in 5 minutes.
If the initial surface coverage is 8.9*10^16 molecules/cm^2, how long will it take for one-half of the film to evaporate? b. What fraction of the film is left after 10 s? Assume the same initial coverage as in part a.
how much product could form assuming no loss of grignard reagent to side reactions and addition of excess benzophenone.
Given the following heats of formation, delta H f, in kJ per mole, as obtained from a table of deltaHf data, calculate the delta H for the reaction in part f. Compare your answer with the result you obtained in Part e.
Estimate Keq for the following equilibria at 425 K. Note that H2O is present as a gas rather than as a liquid. R = 8.3149 J/(mol*K).
Using this equation, determine how many moles are formed for every one mole of KIO3. KIO3 + 5I + 6H ? 3I2 + 3H2O + K B)Using this equation, determine how many moles S2O3 are needed to titrate the number of moles of I2 calculated in A.
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