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Given: The air pollutant NO is produced in automobile engines from the high-temperature reaction: N2(g)+O2(g)<=>2NO(g), Kc=1.7x10^-3. Question: Calculate the equilibrium concentrations if the initial concentrations are 2.31M N2 and 0.54M O2. (This N2/O2 concentration ratio is the ratio found in air.)
a metal weighing 50.0g absorbs 220.0 J of heat when its temperature increases by 120.0 degrees celsius. what is the specific heat of this metal?
7.65.50 mL of 0.161 M HF is titrated with 0.1200 M NaOH. What is the pH after 65.50 mL of base have been added? (Ka for HF is 6.8 x 10-4)
Compute the number of moles - As we know many volatile substances are present in Earth's atmosphere in trace amounts.
Descibe at least four possible factors which may influence the amount of light absorbed by a solution and how these factors may affect the absorption
Find out how many total moles of gas are produced If a sample has 2.10 mL of nitroglycerine (density = 1.592 g/mL) is detonated?
How many grams of NaNO2 form when 429 g NaNO3 react? The yield is 90.%.
Acetylene gas (C2H2) is produced as a result of the reaction CaC2(s) + 2 H2O(l) → C2H2(g) + Ca(OH)2(aq).
If an automobile is able to travel 247 mi on 10.8 gal of gasoline, what is the gas mileage in km/L.
If a reaction mixture initially contains 443 of and 391 of , what is the mole fraction of when equilibrium is reached.
60.0 mL of a 0.450 M HNO_3 solution is titrated with 0.570 M KOH. Calculate the volume of KOH required to reach the equivalence point.
What is the minimum number of liters of air that must pass over a sample of the compound at 25oC to vaporize 1.0 mg of it? Hint: You know the Vapor Pressure from question "a" above and you are given the temperature and mass.
Calculate the standard heat of reaction, or for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero.
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