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How many electrons can be removed from element 69 before it is reduced to its core electron configuration? For the purposes of this question, the core electron configuration is the configuration of the next lightest rare gas atom.
Calculate the equilibrium concentrations if the initial concentrations are 2.31M N2 and 0.54M O2. (This N2/O2 concentration ratio is the ratio found in air.)
A compound of iodine and cesium contains 63.94g of metal and 61.06g of nonmetal. How many grams of cesium are in 38.77g of the compound? How many grams of iodine?
2.0 L of gas A at 1.0 atm and 1.0 L of gas b at 1.0 atm are combined in a 3 L flask. The flask is sealed and over time they react to completely to give gas C according to 2A(g) + B(g)= C(g)
Sulfur dioxide reacts with chlorine at 227 oC: SO2(g) +Cl2(g) ↔ SO2Cl2(g) Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction vessel.
particular sample of pure iron requires 0.595 kj of energy to raise its temperature from 25oc to 45oc. the specific
If 84 g of CO reacts to produce 63 g of CH3OH, What is the percent yield of CH3OH?Answer in units of % ?
Outline the steps necessary to properly prepare 100ml of TE buffer. Include the amounts of Tris-base and EDTA, and all steps necessary to adjust the pH, including when you add what bolumes of water.
A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask
which phase transitions more likely to occur?
Given the following at 25°C and 1.00 atm: 1/2N2(g) + O2(g) ® NO2(g)DH0 = 33.2 kJ N2(g) + 2O2(g) ® N2O4(g)DH0 = 11.1 kJ Calculate the DH0 for the reaction below at 25°C. 2NO2(g) ® N2O4(g)
What is the concentration of H2SO4 present if 42.3 mL of the base is needed to reach the equivalence point?
What is the change in internal energy (in J) of a system that absorbs 0.603 kj of heat from its surroundings and has 0.903 kcal of work done on it
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