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Rhodium has a density of 12.41 g/cm3 and crystallizes in a face-centered cubic lattice. Calculate the radius of a rhodium atom?
The numbers above are also the only numbers I am given. I do not have delta G's of molar G's. If you have an answer that solves for the G's and shows me step by step how to solve the problem, you will get five stars.
What are the n and l quantum numbers of the electron removed when Bi is ionized to Bi+ and would you expect element 115 to have ionization energy greater than, equal to, or less than that of bismuth? Explain.
Calculate the number of mmoles of primary standard grade Na2CO3. b. How many mmoles of HCl reacted with the Na2CO3? c. Calculate the molarity of the HCl solution.
If the average human body discharges 850 g of CO2 per day, how much NaOH is needed each day for each person in the spacecraft? Answer in units of mol.
If you start with 1.000 g of sulfur (S8) and obtain 4.963 g of pure compound. What is the empirical formula of this compound?
A bottle of nail polish remover contains 182 mL of acetone, how much heat would be released by its complete combustion? The density of acetone is 0.788mL.
Draw a series of titration curves for the titration of a strong base with a strong acid where the concentration of the acid is 10 -1 , 10 -2 , and
Ethylene glycol, C2H6O2 (MW=62.1mol) has a density of 40.0 mass percentage and a solution of ethylene glycol in water is 1.0514 g/mL at 20 EC. Calculate the molality of the solution
volumetric flask and this solution becomes quite warm, but after it is permitted to return to room temperature, H 2 O is combined to total 500 mili litres of solution. Compute the pH of the final solution. ?
Barium metal crystallizes in a body centered cubic lattice. the unit cell edge length is 502 pm and the density of the metal is 3.50g/cm3. using the information, calculate the avogadros number. assume 68% of the unit cell is occupied.
Calculate E when 900.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol*K
One way to isolate metals from their ores is to react the metal oxide with carbon as shown in the following reaction: 2MO(s) + C(s) → 2M(s) + CO2(g)
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