Compute the mass of nitrogen dissolved
Calculate the mass of nitrogen dissolved at room temperature in an 94.0 home aquarium. Assume a total pressure of 1.0 and a mole fraction for nitrogen of 0.78.
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A 0.670 Liter can of CO2 gas at 273 K and 1 ATM of pressure is thrown into dry ice. The temp falls to 50 K and the volume decreases to 0.1 L after the can collapses. What is the pressure after the can collapses?
1.00 mol C_12_H_22_O_11_ is added to .150 kg of water and the water is heated to 100 degrees celsius. What is the vapor pressure of the solution at this temperature in mm Hg?
The photosynthesis reaction is 6CO2(g)+6H2o(g)-> C6H12O6(s)+6O2(g). If the reaction requires 2.82^3 kJ/mole of C6H12O6 formed: How many grams of C6H12O6 can be produced from 6.20x10^5kJ?
When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?
Ammonia and hydrazine are both compounds of nitrogen and hydrogen.Based on the law of multiple proportions, how many grams of hydrogen would you expect 3.47 of nitrogen to combine with to yield ammonia?
Metallic aluminum reacts with MnO2 at elevated temperatures to form manganese metal and aluminum oxide. A mixture of the two reactants is 67.2% mole percent Aluminum. Find the theoretical yield (in grams) of manganese from the reaction of 270 gram
An ice cube is placed in a beaker of water at 20 c. the ice cube partially melts and the temp of the water is lowerd to 0 c at this point both ice and water are at0 and no further change is apparent.
The boiling point of a solution containing 10.44 g of an unknown nonelectrolyte in 50.00 g of acetic acid is 159.2°C. What is the molar mass of the solute?
We have a solution that contains 0.022 M Ca2+ and 0.014 M Mg2+. We will use potassium hydroxide to selectively precipitate one of the ions, while leaving the other ion in solution.
If 12.5 g of iron(III) oxide (rust) are pro- duced from 8.74 g of iron, how much oxygen gas is needed for this reaction?
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