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Using Hard-Soft Acid-Base Theory, classify each of the species in the following equilibrium as hard or soft and indicate whether reactants or products will be favored in each of the following equilibria by circling the appropriate species:H2S + HgO <>H2O + HgS
a cylinder of compressed gas has a pressure of 4.882 atm on one day. the next day the same cylinder of gas has a pressure of 4.690 atm, and its temperature is 8 degrees celcius. what was the temperature on the previous day?
The density of a 23.0% by mass ethylene glycol (C_2 H_6O_2) solution in water is 1.03 g/mL. What is the molarity of the solution?
A nugget of pure gold of 4.80 grams absorbed heat of 283 Joules. if the temperature was 23.0°C initially then determine what was the final temperature of the Au gold it is given that the specific heat of Au= 0.129 J/(g·°C).
Assuming Kf= 478Kg/s^2, calculate and compare the fraction of molecules in the first excited vibrational state at 1000K
That is, if you see a second layer of insoluble organic liquid, what could the unknown be in addition to a tertiary alcohol?
One of the steps in the commercial process for converting ammonia to nitric acid is the conversion of ammonia to nitric oxide.
Standard Enthalpies of Formation: acetic and AB2 = - 25.65 kCal/ mole,A++ = -8.65 k Cal/ mole,Temperature = 10 Degree Celsius determine pK,
An aqueous solution of KNO3 has a molal concentration of 1.099 mol kg-1. Its density is 1.0630 g mL-1. Calculate the molar concentration of KNO3.
1)WhenH2(g)reacts withC2H4(g)to formC2H6(g),137kJ of energy areevolvedfor each mole ofH2(g)that reacts. Write a balanced thermochemical equation for the reaction with an energy term in kJ as part of the equation.
the sample has a mass of .211 grams,a volume of .25 and a temperature of 275K at a pressure of .945 atmospheres. What is the most likely element forming the sample?
The pH of the solution is 2.81 after 15.00ml of base is added. Calculate the ionization constant,Ka, of lactic acid.
You start with 100.0 mL of a 0.2500 M solution of NaCl sitting in a beaker. After several days you test the solution and find that it is now 0.3125 M. How much water must have evaporated?
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