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Consider the dissolution of CaCl2. CaCl2(s) --> Ca2+(aq) + 2 Cl (aq) H = - 81.5 kJ A 23.5 g sample of CaCl2 is dissolved in water, with both substances at 25.0 °C. Calculate the final temperature of the solution assuming no heat is lost to the surroundings, the final mixture has a mass of 100.0 g and the solution has a specific heat capacity of 4.18 J °C-1 g-1. The molar mass of CaCl2 = 110.98 g/mol.
The relationship (if any) of the lattice energy of compounds such as ZnO vs. H3BO3 vs. their respective solubilities. For instance, at neutral pH and standard conditions
Considering which elements are being oxidized and reduced, determine how many moles of electrons are transferred between the elements being oxidized and reduced
A bottle containing 305 g of cleaning solution is used for carpets. If the cleaning solution has a specific gravity of 0.850, what volume of solution was used?
What would be the structure and name of the open chain hydroxyl/carbonyl compund from which the above hemiacetal might form
Important information about Nitration, Explain why nitration of 1,4-dichloro-benzene yields the mononitro derivative while N,N'-diacetyl-1,4-phenylenediamine forms
Calculate the molar mass of a gas that has a density of 0.232 g/L at 156 oC and 222 torr. Use R = 0.0821 L-atm/mol-K for the value of the gas constant.
When aminobenzene is subjected to standard nitration conditions {HONO2/(HO)2SO2} poor yields 1-amino-3 itrobenzene are obtained.
A flask contains 0.180 mol of liquid bromine, Br_2. Determine the number of bromine molecules present in the flask.
Calculating Delta H, Use some or all of the following reaction enthalpies to calculate delta H for the reaction:
Constant external pressure of3.00 atm, followed by2) against a constant external pressure of 2.00 atm. Calculate q and w. (101.33 J = 1 L atm)
At a temperature T, a previously empty 5.00L flask is prepared by adding 1.20 mol SO2 and 1.5 mol of O2. Determine the concentrations of SO2, O2 and SO3 once equilibrium is established. KC=963
refer to the given equation as 4NH3(g) + 7O2(g) = 4NO2(g) + 6H2O(g) How many moles of ammonia will be required to produce 13.8 mol of water.
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