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Consider the reversible reaction: 2NO2(g)?N2O4(g)^-1 If the concentrations of both NO2 and N2O4 are 0.016 mol • L , what is the value of Qc? The answer is supposed to be 63 but how and why?
how many regions of high electron density are there around the central atom of the molecular structure of SbCl3.
At a certain temperature the equilbrium constant is 396 K for H2(g) + I2(g) ↔ 2HI(g) , Calculate the the equilbrium constant for 0.5H2(g) + 0.5I2(g) ↔ HI(g)
How many total moles of oxygen gas can be generated through this decomposition? B. If this oxygen is formed within the bottle described in question 1, what change in pressure would be predicted?
The pK value of the system is 6.1. If the [CO2] is expressed in terms of partial pressure and equals 1.3kPa and the bicarbonate concentration is 2.2 x 10^-3 M, what is the pH of the solution.
How many atoms of He gas are present in a 450 mL container at 35°C and 740 mmHg
what is the density of 53.4 wt% aqueous NaOH if 16.7 mL of the solution diluted to 2.00L gives 0.169M NaOH
suppose you want to find out how many milliliters of 1.0 M AgNO3 are needed to provide 169.9g of pure AgNO3.
At a certain temperature the vapor pressure of pure benzene and pure toluene are 380 torr and 130 torr, respectively.
A 10.0-mL sample of a HCl solution has a pH of 2.000. What volume of water must be added to change the pH to 4.000?
A solution contains Ba2+ (1.0x10^-3) and Ca2+ (1.0x10^-3). Drops of a 5.0x10^-1 M solution NaF were added using a buret until the [F-] in the solution mixture reached 1.5x10^-3 M.
In an insulated container, a hot piece of iron (cp =0.4513 J/g-C) at 1490. C was added to 200. g of water (cp =4.184 J/g-C) at 20. C. The temperature of the resulting mixture became 90. C. What mass of iron was present?
From the composition of lignite coal, calculate the mass of sulfuric acid that could potentially form as acid rain from burning
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