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A 7.45 g sample of solid LiOH is completely dissolved in 120.00 g of water at 23.25°C contained in a calorimeter with a heat capacity of 11.7 J/°C. The specific heat capacity of the solution produced was 4.20 J/g•°C, and final temperature reached was 34.91°C. How much heat was produced by the dissolution?
Assuming that the loss of ability to recall Chem 401 material is a first-order process with a half-life of 55 days for the traditional (talking head lecture) and a C of 305 days for the active approach,
when burned in oxygen, yielded a mixture of CO2 and SO2 in which the number of moles of CO2 was one-half the number of moles of the SO2. How many grams of C contained in the mixture?
balanced oxidation half reaction and balanced reduction half reaction?
complete the following chart of gas properties. For each positive observation, write a balanced chemical equation to describe the process.
After adding the two portions into the calorimeter setup and following the procedure outlined in the experiment, you determine the temperature of the mixed portions of water to be 45*C. what is the heat capacity of the calorimeter?
A certain reaction has an activation energy of 61.0 kJ/mol and a frequency factor of A1 = 2.00×10^12M^-1s^-1. What is the rate constant, k, of this reaction at 29.0 degrees celsius
Predict the sign of delta S for each of the following changes.
How much heat is required to take a 15.0 g sample of ice with an initial temperature of 0.00oC and raise it to a final temperature of 75.0 oC.
How much heat is required to vaporize 351 g of liquid ethanol at its boiling point.
How would the results differ if you added sodium p-toluate instead of p-toluic acid to the two-layer mixture of tert-butyl methyl ether and water
Apart from the discrete energy values characteristic of a quantum mechanical system, is the result of an invidvidual measurement of the total energy identical to the result obtained on a classical system?
The temperature of the entire system rose from 25.30 °C to 26.59 °C. Calculate the heat of reaction, in kJ, per mole of KOH(aq).
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