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the air in the laboratory was measured with a barometer to be 7.20 x 10 squared mm Hg. what is the laboratory air pressure in atm.
420 g of butane reacts with 1510 g of oxygen to produce 1390 g of carbon dioxide and 652 g of water.What is wrong with this description?
A 75.0-mL volume of 0.200 M NH3(Kb=1.8*10^-5) is titrated with 0.500 M HNO3. Calculate the pH after the addition of 25.0 mL of HNO3.
At 25oC, the acid dissociation constant for hypochlorous acid HOCl is 3.5E-8. Calculate the concentration of the hydronium ion in an aqueous solution of 0.30M HOCl.
Consider an unknown that is approximately 50.% KHP. What mass of the unknown would be required to react with 40. mL of 0.10 M NaOH?
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.
How can I make up 100ml of a solution containing Compound A (solid, purity of 83.7%) at 90 ug/ml and compound B (liquid, density 1.12 and purity of 90.5) at 30 ug/mL for HPLC reference standard.
An experiment shows that a 247 mL gas sample has a mass of 0.432 g at a pressure of 747 mmHg and a temperature of 28 degrees celcius.What is the molar mass of the gas?
what is a detailed mechanism for the formation of dibenzalacetone? This reaction is beginning with acetone and benzaldehyde and is treated with NaOH and then forms dibenzalacetone.
A feed stream containing a mixture of 40% n-butane, 30% n-pentane and 30% n-hexane flows into a flash unit. The flash temperature is 290 K and the flash pressure is 0.6 bar
a pH meter measures the concentration of hydronium ions, H3O+ in solution through the creation of a concentration differential between a standard hydrogen half cell inside the pH probe and the concentration of hydronium ions outside the probe
The rate of effusion of a particular gas was measured and found to be 24.0 mL/min. Under the same conditions, the rate of effusion of pure methane (CH4) gas is 47.4 mL/min. What is the molar mass of the unknown gas?
Calculate w (in kJ) when 597 g iron (III) oxide (MM = 159.7 g/mol) reacts with excess carbon to produce carbon dioxide gas at 459 K:
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