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Three bulbs are connected by tubing, and the tubing is evacuated. The volume of the tubing is 50.0 mL. The first bulb has a volume of 88.0 mL and contains 4.63 atm of argon, the second bulb has a volume of 250 mL and contains 1.69 atm of neon, and the third bulb has a volume of 30.0 mL and contains 4.96 atm of hydrogen. If the stopcocks (valves) that isolate all three bulbs are opened, what is the final pressure of the whole system in atm?
A certain mass of oxygen was collected over water when potassium chlorate was decomposed by heating. The volume of the oxygen sample collected was 870 mL at 40C and a barometric pressure of 755 torr.
A reaction has a theoretical yield of 8.83 g of ammonia. the reaction gives off 10.24 L of ammonia measure at 52*C and 105.3kPa what was the percent yield of the reaction?
At 10 degrees, Kc = 56.3 for the reaction below. H2 + Cl2 --> HCl
How much heat is required to raise the temperature of 7.50 grams of water from 10 degrees celcius to 55 degrees celcius
How many liters of oxygen collected over H2O and measured at 27 degrees Celsius and 745.0 mm Hg can be prepared by decomposing 4.421 grams of gold (III) oxide? The vapor pressure of H2O at 27 degrees Celsius is 26.7 mm Hg.
Calculate the voltage of the cell 2Ag+(aq) (0.200 M) + Cu(s) Cu2+(aq) (0.080 M) + 2Ag(s) Eocell = 0.460 V
A gas originally at 27 degrees celsius and 1.00 atm pressure in a 3.9 L flask is cooled at constant pressure until the temperature is 11 degrees celsius. determine the new volume of the gas and express your answer in Litre.
A 33.0 g sample of a nonelectrolyte was dissolved is 700. g of water. The solution's freezing point was -2.84°C.
For the reaction SO3+H2O=H2SO4 calculate the percentage yield if 600 g of sulfur trioxide react with excess water to produce 475 g of sulfuric acid
Assume that algae need carbon, nitrogen and phosphorus in the atomic ratio 106:16:1. What is the limiting nutrient in the lake that contains the following concentrations: total carbon = 20 mg/L, total N = 0.80 mg/L and total P = 0.16 mg/L.
A solution is prepared by mixing 87.0 mL of 5.00 M HCl and 36.0 mL of 8.00 M HNO3. Water is then added until the final volume is 1.00 L. Calculate [H+ ], [OH - ], and the pH for this solution.
One mole of an ideal gas with Cv,m = 3R/2 initially at 325K and 1.5*10^5 Pa undergoes a reversible adiabatic compression. At the end of the process, the pressure is 2.50 * 10^6 Pa.
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