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A 0.692 g sample of glucose, C6H12O6, is burned in a constant volume, bomb calorimeter. The temperature change is measured at 1.80 degrees C. The calorimeter contains 1.05 kg and the "dry" calorimeter has a heat capacity of 650. J/ degrees C. Calculate the amount heat evolved per mole of glucose.
The rate of the reaction will increase if the pressure of the gases increases. The rate of the reaction will remain constant with increasing temperature. The rate of the reaction will increase as time increases.
Suppose you measured the pressure with a barometer which was not vertical. You measured the pressure to be 752mmHg and then noticed the barometer
The standard free energy for the neutralization of HCl with NaOH at 25 degrees celsius is -79.9KJ/mol. Calculate the equilibrium constant for the reaction.
A sample of 40.0 ml of a .1 M acetic acid solution is titrated with .150 molar sodium hydroxide Ka for acetic acid is 1.8 x 10^-5. What is pH of solution at equivalence point
Write a balanced equation including states of matter for the reaction of Zn(H2O)4 2+ in aqueous NaCN. You can assume sodium is a secator ion and does not need
An auto bumper is coated with a layer of chromium, 0.017 cm thick. The bumper has a surface area of 3.43 x 104 cm2. The density of chromium metal is 7.19 g/cm3. How many atoms of chromium are used in the coating?
at 700 k the equilibrium constant for the reactionccl4g ltgt cs 2 cl2gis kp 0.76. a flask is charged with 2.00 atm
lead to two products. Draw the major product that is observed in practice, as well as the preceding intermediate.
4388 M KOH solution reacts with 50.60mL of CH3COOH solution, what is the molarity of the acid solution?
calculate w for the following reactions that occur at 298k and 1 atm pressure, CO2(g) + NaOH(s) -> NaHCO3(s) and 3O2(g) -> 2O3(g)
evaporate more quickly: 55 mL of water in a beaker or 55 mLmof acetone in an identical beaker under identical conditions?
(NH4)2Cr2O7(s) ? N2(g) + 4 H2O(g) + Cr2O3(s) If 0.95 g of ammonium dichromate is used and the gases from this reaction are trapped in a 15.0 L flask at 23 °C, what is the total pressure of the gas in the flask. What are the partial pressures of N2..
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