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The density of copper metal is 8.95g/cm3. Explain if the radius of a copper atom is 127.8 pm, is the copper unit cell simple cubic, body centered cubic, or face centered cubic?
Dry ice is solid carbon dioxide. A 1.87g sample of dry ice is placed in an evacuated 4.03 L vessel at 22 degrees C. Calculate the pressure inside the vessel after all the dry ice has been converted to CO2 gas
Describe how you would prepare the following aqueous solution: 230 g of a solution that is 0.60 molal Na2CO3 starting with the solid solute.
Calculate K for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give dinitrogen tetroxide gas
2NaN3(s)--> 2Na(s) + 3N2(g) How many grams of sodium azide are required to produce 19.00L of N2 at 273K and 775mmHg. A) 34.9 B) 52.0 C) 2.66*10^4 D) 3.89*10^5 E) 5.80*10^5
Calculate the heat of the reaction for the sample (kJ). Calculate the heat of the above reaction in J/mol of HCl.
A protein contain the following amino acids 61 LYS 75 GLU 26 TYR 22 HIS 45 PRO 47 PHE 29 ARG 67 GLY 77 ASP 65 ALA 24 THR 25 MET 71 VAL 56 ILE 12 SER 83 LEU A) What is its net charge at pH 13
Explain why it could be a health hazard to improperly smell a chemical in the laboratory.
Predict if the following conditions would result in the formation of a precipitate, explain briefly: a) 0.0025 M Fe 3+ at pH 6.00
At 1478 oC the equilibrium constant for the reaction: 2 IBr(g) ? I2(g) + Br2(g) is KP = 0.899. If the initial pressure of IBr is 0.00169 atm, what are the equilibrium partial pressures of IBr, I2, and Br2? p(IBr) = . p(I2) = . p(Br2) = .
Measurements also show that a certain sample of the unknown compound contains 9.8 mol of oxygen and 3.31 mol of chromium.
Determine the pH at the equivalence (stoichiometric) point in the titration of 30.9 mL of 0.804 M HCOOH by 0.369 M LiOH. The Ka of HCOOH is 1.8 x 10-4.
Without referring to a table, select from the following list the gas that has the largest value of b in the van der Waals equation: CH4, O2, H2O, CCl4, Ne.
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