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Consider the following reaction. H2O(g) + CO(g) H2(g) + CO2(g) In a particular experiment 1.0 mol H2O(g) and 1.0 mol CO(g) are put into a flask and heated to 350°C. In a second experiment 1.0 mol H2(g) and 1.0 mol CO2(g) are put into another flask with the same volume as the first. This mixture is also heated to 350°C. After equilibrium is reached, will there be any difference in the composition of the mixtures in the two flasks? yes no Explain.
Preparation of and alpha, beta-unsaturated ketone via Michael and Aldol Condensation: 6-ethoxycarbonyl-3,5-diphenyl-2-cyclohexanone.
Identify the most important types of interparticle forces present in the solids of each of the following substances: A) BaSO4 B) H2S C) Xe D) C2H6 E) CsI F) P4 G) NHs
Assuming the oil layer to be one molecule thick, calculate the approximate diameter in Angstroms (1 A = 10^-10 m) of a single molecule. (Use volume = area x depth.)
Describe, in detail, the structure of ATP and its function in oxidative phosphorylation and photosynthesis
Calculate the partial pressure of water at 23.6 Celsius by interpolation from the vapor pressure table.
A 46.2mg sample of phosphorus reacts with selenium to form 135mg of the compound. What is the empirical formula of the phosphorus selenide
liquid mercury at atmospheric pressure and 298K to 1.25L at constant temperature requires 46.6kbar (kilobars) of external pressure. What is the isothermal compressibility of Hg(l)?
If the pressure exerted by ozone, in the stratosphere is 3.0*10^-3 atm and the temperature is 253 K, how many ozone molecules are in a liter?
A water sample is analyzed for a pollutant by the standard addition method . four solutions are prepared,each with a 10.00 ml aliquot of the water sample and varying amounts of a 10 ppm standard solutions of the pollutant
What is the molar solubility of CaF2 in 0.10 M NaF solution at 25°C? The Ksp for CaF2 is 1.5x10^-10.
Describe the preparation of a 1.50 M, pH 8.0 tris buffer (500 mL) using tris base (MW= 121.1 g/mol) and 3.0 M HCl. pKa of tris is 8.3
When 1.269 g of this compound (molar mass = 103.67 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.029 °C. What is the heat capacity (calorimeter constant) of the calorimeter
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