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If the coal is burned in a power plant that uses 1800 tons of coal per day, what mass of calcium oxide is required daily to eliminate the sulfur dioxide?
A balloon with an initial volume of 3.8 L at a temperature of 305 K is warmed to 385 K. What is its volume at the final temperature?
The disinfectant hydrogen peroxide (H2O2) decomposes to form water and oxygen gas.How much O2 will result from the decomposition of 3.21 mol of hydrogen peroxide?Answer in units of mol.
A certain reaction, a+b=c is the first order with respect to each reactant, with k=1.0x10-2l.mol-1s-1. Calculate the concentration of A remaining after 100s if the initial concentration
If 4.10 mol calcium carbide (CaC2) reacts with an excess of water, how many moles of acetylene (C2H2) will be produced?
a sample of gas occupies 12 liters under a pressure of 1.2 atm. what would its volume if the pressure were increased to 2.4 atm? assume the the temperature of the gas does not change.
A 125 mL sample of dry air at 230 degrees celcius is cooled to 100 degrees celsius at constant pressure. What volume will the dry air occupy at 100 degrees celsius.
Compression and Cooling of Nitrogen Gas. A volume of 65.0 ft^3 of N2 gas at 90°F and 29.0 psig is compressed to 75 psig and cooled to 65°F.
determine the molecule weight of the liquid and the density of the vapor under these condition?
A solution is prepared by dissolving 396 g of sucrose (C12H22O11) in 624 g of water. What is the vapor pressure of this solution at 30°C? (The vapor pressure of water is 31.8 mmHg at 30°C.)
Write the net ionic equation for the following reactions: a. The precipitation of manganese (II) hydroxide b. The reaction that occurs when sodium fluoride is added to a solution containing iron
In Europe, gasoline efficiency is measured in km/L . If your car's gas mileage is 30.0 miles/gal, how many liters of gasoline would you need to buy to complete a 284- km trip in Europe?
For the concentration of hydroxyl radical of 7.5E06 molecules/cm3 and a carbon monoxide concentration of 18 ppm, calculate the rate of its reaction with atmospheric carbon monoxide at 11 degrees C.
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