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Calculate the heat energy released when 19.6 g of liquid mercury at 25.00 °C is converted to solid mercury at its melting point.
Changing the conditions of the reaction can alter the value of the change in free energy (?G). Sort the following conditions as to whether each would decrease the value of ?
What is the maximum number of electrons in an atom that can have the following set of quantum numbers?
An 85.0g sample of iron requires 954 J of heat to raise its temperature 25.0C. What is the specific heat of the iron?
what is the delta Hrxn, delta Grxn and delta Srxn at 298 K. Ethylbenzene, C6H5--CH2CH3 : delta Ht = -12.5 kJ/mol, delta Gt = 119.7 kJ/mol and S = 255 J/mol*K Styrene, C6H5--CH==CH2 : delta Ht = 103.8 kJ/mol, delta G..
Ammonia condenses to form a liquid at -33.35C at atmospheric pressure. The density of liquid ammonia at this temperature is 0.6818g/ml. If the ammonia (0.224ml) is condensed at these temperatures, what would be its volume?
Dry the hydrate as instructed in the lab procedure, noting down it's mass until it appears to no longer decrease (no more water bound in the sample).
If 45.8 grams of aluminum metal are reacted with excess HCl, what volume of H2 gas would be generated at 23.0 ºC and 1.00 atm pressure?
Two moles of a monoatomic gas are contained atpressure 1 atm and teperature 300 k. 34, 166 joules of heat are transfered to the gas as a result the gas expands and does work on the surroundings of 1214 joules.
A solution is made by dissolving 0.100 mols of NaOCl in 100.0 mL of water. The Ka of hypochlorous acid (HClO) is 3.0*10^-8 at 25.0 degrees C.
A gaseous mixture of O2 and N2 contains 36.8 nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 545 mmHg ?
If the combustion gases consist of CO2, H2O, CO, O2, and N2 that exit at 1200 K and 2 atm, determine (a) the equilibrium composition of the product gases and (b) the rate of heat transfer from the combustion chamber. Is it realistic to disregard t..
When 5.00 × 1022 molecules of ammonia react with 4.00 × 1022 molecules of oxygen, how many grams of nitrogen gas are produced? 4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g)
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