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The change in enthalpy Delta H for a reaction is -39.6 kJ/mol. The equilibrium constant for the reaction is 4.4×103 at 298 K.What is the equilibrium constant for the reaction at 635 K?
A buffer initially contains 0.10 mol acetic acid and 0.13 mol of sodium acetate in 1.00 L. 0.02 mol of potassium hydroxide is added to the buffer
A sample of vanadium haveing 5.67 grams of mass upon heating combined with oxegen of 4.45gramsto make vanadium oxide. Determine the emperical formula for this compound?
Acid, Bases and Proton Transfer, what is the direction of proton transfer?
Enter the sign of H° and S° for the condensation for CO2. Enter the sign as either + or -. Also indicate the temperature conditions (high temperature or low temperature) that favor condensation of CO2
In a calorimeter, 10 g of ice absorbs heat with an enthalpy of fusion of 334 J/g. What is the heat absorbed.
Calculate the fraction of atoms in a sample of argon gas at 360. K that have an energy of 14.0 kJ or greater.
Suppose that in changing samples, a portion of the water in the calorimeter weere lost. In what way, if any, would this change the heat capacity of the calorimeter?
A 33.0 g sample of a nonelectrolyte was dissolved is 700. g of water. The solution's freezing point was -2.84°C.
What would you expect to observe when adding one drop of iodine-potassium iodine reagent to each of the four carbohydrates?
How many moles of ammonia will be required to produce 10.0 mol of water
Working with Temperature and Gas 1. What is the final temperature if 25 mL of milk 3.0 degrees Celsius is mixed with 150 mL of coffee at 95 degrees Celsius? Start by writing the equation that shows conservation of energy. State any assumptions you..
Calculate the expected change in temperature for 4.5 g of NH4NO3 dissolved in 100.0 mL of H2O. Assume that the calorimeter absorbs no heat.
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