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1.50 g of nh3 react with 2.75g of o2 which is the limiting reactant? How many grams of excess remain after the limiting reactant is completely consumed?
What is the most important type of intermolecular attractive force that operate in each
What mass of carbon dioxide is present in 1.00m^3 of dry air at a temperature of 25c and a pressure of 731torr? Calculate the mass percentage of oxygen in dry air.
If the atmospheric pressure at 30 km is 28.0 torr and the temp is -48 C, what is the volume of the balloon when it bursts?
calculate the pH of a solution formed by mixing 65 mL of .27 M NaHCO3 with 75 mL of .12 M Na2CO3
what is the value of Kp for this reaction at this temp? what wold be the effect of an increase in pressure on the amount of SO_3 produced? what wold the effect of an increase in temp on the amount of SO_3 produced? (use relevant data from Appendix..
the mass of water is 92.6 grams, the initial temperature of the water is 58.9 degrees celsius, the mass of teh liquid nitrogen added to the water is 57.1 grams, and the final temperature after the liquid nitrogen has vaporized is 29.6 degrees cels..
Find the pH of a solution prepared by dissolving all of the following compounds in one beaker and diluting to a volume of 1.00 L: 0.180 moles acetic acid (pKa=4.75), 0.180 mole sodium acetate
when 8.00g of NaOH is added to a calorimeter filled with 75.0mL of HCl the temperature of the solution increases for 25.0 C to 33.5 C. calculate the molar heat of neutralization for the NaOH. (assume that the density of the solution is 1.00gmL)
You have 170. mL chlorine trifluoride gas at 669 mmHg and 45°C. What is the mass (in g) of the sample?
The Henry's law constant for helium gas in water at 30°C is 3.7 10-4 M/atm; that for N2 at 30°C is 6.0 10-4 M/atm. If the two gases are each present at 1.2 atm pressure, calculate the solubility of each gas. What is the Molarity of He and N2
Calculate the mass of silver chloride required to plate 295mg of pure silver.
Assume that the wet limestone process requires 1 metric ton of calcium carbonate to remove + 85.0 % of the sulfur from 4 metric tons of coal containing + 10.0 % S Assume that the sulfur product is calcium sulfate.
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