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An empty 2.0 L soda bottle is tightly capped at 22 degrees Celsius and 650 mmHg. If the bottle is placed in water at 95 degrees Celsius, what is the pressure in the bottle?
The solution to Equilibrium constant, A certain gas mixture held at 395C has the following initial partial pressures: P(Cl2) = 351.4 torr; P(CO) = 342.0 torr and P(COCl2) = 0.
One beaker contains 10.0 mL of acetic acid/sodium acetate buffer at maximum buffer capacity (equal concentrations of acetic acid and sodium acetate), and another contains 10.0 mL of pure water.
Petroleum consumption in the US in 1990 supplied about 34.6E15 kJ of energy. Of this quantity, about 14.3E15 kJ was supplied by foreign sources.
how many liters of H2 would be formed at 530 mm Hg and 15 degrees celcius if 20.5g of zinc was allowed to react?
Why does the same amount of liquid when left in a wider and flatter container evaporate quicker than when left in a narrower and deeper container?
Calculate the molar enthalpy of combustion of Phosphorous when this combustion process was carried out under the constant pressure?
Consider two solutions. One solution is 0.1115 M Ca(OH)(2). The other is 0.1050 M HClO(4). a) Write a balanced equation for the reaction between the two solutions.
what is the total pressure in a canister that contains oxygen gas at a partial pressure of 804 mm Hg, nitrogen at a partial pressure of 220 mm Hg, and hydrogen at a partial pressure of 445 mm Hg.
Compute pH and [OH-] for each of the following solutions. (a) 8.1×10-2M Na2CO3, (b) 0.15M NaCN
Chemical Reactions explained in this solution, 1. Some sulfuric acid is spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric ac..
Concentrations of Components in an Equilibrium, The following equilibrium process at 686 deg. C. CO2(g) + H2(g) f/r CO(g) + H20 (g)
A cube of osmium metal 1.500cm on a side has a mass of 76.31g at 25°C. Calculate the mass of 0.1500L of benzene at this temperature.
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