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Five 5.00ml samples of 1.0 M reagent B were poured into five vessels containing 5.00ml of A, each having the concentration tabulated below. The temperature was 25 degrees Celsius and all other conditions were constant. The initial rates are also tabulated. Another set of experiments was performed in which the concentration of B was varied- these results are also tabulated.
conc A Conc B Initial Rate Conc A Conc B Initial Rate1.0 1.0 0.012 1.0 1.0 0.0122.0 1.0 0.023 1.0 2.0 0.0484.0 1.0 0.049 1.0 4.0 0.1908.0 1.0 0.096 1.0 8.0 0.76016.0 1.0 0.190 1.0 16.0 3.0
Given this information, what is the order of reaction with respect to A and with respect to B? What is the value of the rate constant?
A reaction takes place at a constant pressure of 1.10 atm with an internal energy change of 71.5 kJ and a volume decrease of 13.6 L.
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2.00 moles of a gas occupies 62.2 L at a par- ticular temperature and pressure. Its density is 0.900 g/L. What is the molar mass?
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If a nonvolatile, yellow crystalline solid sample of 0.351 g is dissolved in benzene (C 6 H 6 ) of 15.8 g formed a solution. this solution freezes at the temperature of 4.77 degree celsius.
What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of aqueous hydrofluoric acid requires
The enthalpies of formation of oxalic acid in the solid and aqueous phases are -826.8 and -818.8 kJ/mol, respectively. The heat capacity of water is 4.184 J/g*K. Ignore the heat capacity of oxalic acid.
The pKb values for the dibasic base B are pKb1 = 2.1 and pKb2 = 7.8. Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.75 M B(aq) with 0.75 M HCl(aq).
The heat of vaporization of 1.0 mole of water at 100°C and 1.0 atm is 40.6 kJ. Calculate the change in entropy for the process H2O(l) → H2O(g). Document your work here.
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