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You have a 1.23-mol sample of water at ?30.°C, and you heat it until you have gaseous water at 140.°C. Calculate q for the entire process. Use the following data.
specific heat capacity of ice = 2.03 J °C-1 g-1
specific heat capacity of water = 4.18 J °C-1 g-1
specific heat capacity of steam = 2.03 J °C-1 g-1
H2O(s) ? H2O(l) ?Hfusion = 6.01 kJ/mol (at 0°C)
H2O(l) ? H2O(g) ?Hvaporization = 40.7 kJ/mol (at 100.°C)
The rate constant for a certain chemical reaction is 0.00250 M1 s1 at 25.0C and 0.0125 M1s1 at 50.0C. What is the activation energy for the reaction, expressed in kJ mol?
How many moles of NaF must be added to 100.00mL of 0.15 M HF to prepare a buffer with pH=3.30. Ka(HF)=7.1*10^-4
How many moles of oxygen are combined with 4.20 moles of chlorine atoms in C2O7?
What is the concentration of ammonia in a solution if 21.80 mL of a 0.1160 M solution of HCl are needed to titrate a 100.0 mL sample of the solution?
What is the pH of Na3PO4. While this is a triprotic species, you may ignore two of the Ka's and concentrate on the single Ka that is appropriate for this problem.
A certain substance has a heat of vaporization of 74.45 kJ/mol. At what Kelvin temperature will the vapor pressure be 6.50 times higher than it was at 287 K
The enthalpy of fusion of methanol (CH3OH) is 3.16 kJ/mol. How much heat would be absorbed or released upon freezing 25.6 grams of methanol?
48.61 g of magnesium was dissolved in diluted sulfuric acid and 490 g of MgSO4 . 7H2O was isolated from the solution. How many percent of impurities (if any) did the metal contain?
Explain the characteristics of a single, double, and triple bonds including why they form
Some species with two oxygen atoms only are the oxygen molecule, O2, the peroxide ion, O2-2 , the superoxide ion, O2-1 , and the dioxygenyl ion, O2+1 . Draw an MO diagram for each, rank them in order of increasing bong length, and find the number ..
The aqueous electrolytic solution (d= 1.230 g/cm^3) in a typical automotive battery contains approximately 368 g of hydrogen sulfate (H2SO4, sulfuric acid, MM= 98.07948 g/mol) per liter. Calculate the following concentrations
A sample of fluorine gas occupies 855 mL at 710 mm Hg and 1550C. What is the mass of the sample?
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