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The enthalpy of formation of ethanol, C2H5OH, is -277.0 kJ/mol at 298.15k. calculate the enthalpy of combustion of one mole of ethanol, assuming that the products are CO2 (g) and H2O.
Important information about pH and Molarity, You add 5 drops of .100 M HCl to 100ml of "pure" water. Assuming that the volume of one drop is .035ml, calculate the expected pH of the resulting solution
What is the final dilution obtained after each dilution series shown below? Express each answer in exponential numbers.
How much heat is required to warm 221 g of ice from -44.9°C to 0.0°C, melt the ice, warm the water from 0.0°C to 100.0°C, boil the water, and heat the steam to 173.0°C?
In an equilibrium mixture the partial pressures of SO 2 and O 2 are 0.125atm and 0.460atm , respectively. What is the equilibrium partial pressure of SO 3 in the mixture?
If 5.40 mol calcium carbide (CaC2) reacts with an excess of water, how many moles of acetylene (C2H2) will be produced?
The total molarity of acid and conjugate base in this buffer is 0.100 M . A student adds 6.10 mL of a 0.380 M solution to the beaker. How much will the pH change?
what is the molarity of a solution of sodium hydroxide that contains 47.0 g of naoh in 205.0 ml of solution? use a
You need to produce a buffer solution that has a pH of 5.06. You already have a solution that contains 10 mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? T..
Assuming the solution has a heat capacity of 4.18 J/°C·g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
Name those that have a trisubstituted ring where the methyl gorups are oriented Ortho for 3 different isomers.
If the original sodium tartrate solution had a concentration of 1.00 M instead of 0.100 M, what would the concentration of copper be in a solution created by combining 10 mL of it with 10 mL of the 0.100 M copper (II) sulfate solution.
At a higher temperature, 373K, dinitrogentetraoxide partially decomposes according to the same equilibrium reaction but with slightly different results. The chemical equation is again
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