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175g pure H2O was placed in a constant-pressure calorimeter and chilled to 10C 9.8g pure H2SO4 (also 10C) was added, stirred and the temperature rose to 19.8C.
a)What do we assume about specific heat?b)Calculate the energy change for the reaction.c)What state function does this energy represent?d)Calculate the energy change in kJ/mole.
You have 1005.3 g of a bleach solution. The percent by mass of the solute sodium hypochlorite, NaOCl, is 3.62%. How many grams of solvent are in the solution?
What is the energy of a C-C bond in kJ/mole? Explain. How does this amount of energy compare?
A 4.50-g sample of LiCl at 25.0 C dissolves in 25.0 mL of water also at 25 C. The final equilibrium temperature of the resulting solution is 60.8 C.
How many milliliters of 4.21 M NaOH are needed to completely neutralize 76.9 mL of 0.340 M H3PO4?
Solid silicon and solid magnesium chloride form when silicon tetrachloride gas reacts with magnesium metal. Write a word equation and an unbalanced formula equation. Include all of the appropriate notations.
63.0 mL of a 1.20 M solution is diluted to a volume of 208 mL. A 104-mL portion of that solution is diluted using 157 mL of water. What is the final concentration.
how many grams of urea must be added to enough water to obtain 115 ml of a solution with an osmotic pressure of 2.7 atm at 35 degrees celsius
Find what is the initial concentration of the chlorine before dilution - unknown concentrated chlorine
Consider a glass of 254 mL of water at 25°C. Calculate the mass of ice at -15°C that must be added to cool the water to 10°C after thermal equilibrium is achieved.
CO(g) + 2H2(g) = CH3OH(g) , what is the equilibrium constant? , where CH3OH = 0.0412 atm, H2 = 0.274 atm, CO = 0.914 atm.
Consider a cylindrical container partially filled with ethanol (C2H6O). Using the model in which ethanol vapor pressure is a result of equilibrium between the rate of ethanol evaporation and condensation.
A chemist dissolves 284 mg of pure potassium hydroxide in enough water to make up 140 mL of solution. Calculate the pH of the solution.
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