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The reaction is second order in and has a rate constant of 0.0197 at 25.0 . A reaction vessel initially contains 250.0 of 0.118 which is allowed to react to form the gaseous product. The product is collected over water at 25.0 . How much time is required to produce 146.0 of the products at a barometric pressure of 753.7 . (The vapor pressure of water at this temperature is 23.8 .
When you heat baking soda (NaHCO3), it breaks down into sodium carbonate powder (Na2CO3), carbon dioxide and water vapor. Write a correct thermo chemical equation and explain what it tells you about the reaction ( The enthalpy of this reaction is ..
Calculate the standard cell potential at 25 C for the reaction X(s)+2Y+(aq)?X2+(aq)+2Y(s) where ?H? = -651kJ and S = -371J/K.
Determine the energy in joules of a mole of photons coupled with red light of wavelength
assuming an Sn2 reaction mechanism, predict the major organic product(s) of (s)-3,3-dimethyl-2-butanol when reacted with HCl.
Calculate the pH of a buffer made with 0.50M phosphoric acid and 0.75M sodium dihydrogenphosphate. Ka = 7.5 x 10-3.
if a saturated solution of NH4NO3 at 70 degrees Celsius was cooled to 10 degrees Celsius, how many grams of solute will separate if the quantity of the solvent is 98 grams?
Using the equation Fe2O3+2Al-->2Fe+Al2O3, how many grams of Al are needed to completely react with 135 g Fe2O3
if 69 kJ of heat is applied to a 1012 g block of metal, the temperature of the metal increasesby 11.4 degrees C. Calculate the specific heat capacity of the metal in J/g degrees C.
Calculate the change in entropy (deltaS) when one mole of diamond is heated from a temperature of 0 K to 400 K at a constant pressure of 1 bar
What is the electron configuration for Cuprous and Cupric, and since this is an exception to Aufbau, where are we removing electrons
An analyst was attempting to determine the percent KHP in an unknown sample. The analyst found the molarity of the standardized NaOH solution to be 0.1022 mol/L.
Calculate w (in kJ) when 597 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 459 K:
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