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Sulfur dioxide in the effluent gases from coal-burning electric power plants is one of the principal causes of acid rain. One method for reducing SO2 emissions involves partial reduction of SO2 to H2 S, followed by catalytic conversion of the H2 S and the remainingSO2 to elemental sulfur:2 H2 +SO2 => 3 S + 2H2O
a weather balloon holding 22l of gas is released at a pressure of 103kpa and a temp. of 15c. what is the temp. at 10km
A gaseous mixture contains 0.30 mole of co(g), 0.10 mole of H2(g) AND an Unknown amount of CH4(g) in a litre flask. this mixture is in equilibrium at 1200 deg K acc to
The diluted solution is then placed in a spray bottle for application on the desired surfaces. How many moles of luminol are present in 2.00 L of the diluted spray
Using Hess's Law and the enthalpies of fusion and vaporization of WATER calculate the theoretical value of the heat of sublimation of WATER.
A volume of 60.0mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H2SO4). What was the molarity of the KOH solution if 24.7mL of 1.50 M H2SO4 was needed?
Titration of an oxalate sample gave the following percentages of percent oxalate: 12.28%, 12.54%, and 12.24%. Calculate the average and the standard deviation
How many grams of oxygen are required to completely burn 5.90 g of C3H8 in the following unbalanced equation: C3H8(g) + O2(g) --> CO2(g) + H2O(g)
1.given that the density of a solution of h2so4 is 1.1548 then calculate the molality of a 1.94 wt solution of
How many microcoulombs are required for complete oxidation of glucose in 0.300 microliter of blood in a home glucose monitor if the concentration is 1.00 g/L
Write the balanced equation for the net cell reaction for the voltaic cell in acidic solution. (First two are the anode, last two are the cathode)
What is the change in internal energy (in J) of a system that absorbs 0.535 kJ of heat from its surroundings and has 0.362 kcal of work done on it
39 grams of C6H6 are mixed with 136.6 grams of O2 and allowed to react. How much CO2 could be produced by this reaction?
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