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Consider the following reaction in a closed reaction flask. If 1.50 atm of gas A is allowed to react with 0.500 atm of gas B and the reaction goes to completion at constant temperature and volume, what is the total pressure in the reaction flask at the end of the reaction? What are the partial pressures of the gases in the flask?
4A(g) + 6B(g) ? 2A2B3(g)
A. (0.750 atm A2B3 produced) + (0.25 atm B remaining) = 1.00 atm total pressureB. (0.167 atm A2B3 produced) + (1.17 atm A remaining) = 1.34 atm total pressureC. (1.50 atm A2B3 produced) + (0.167 atm A remaining) = 1.67 atm total pressureD. (0.333 atm A2B3 produced) + (0.500 atm A remaining) = 0.833 atm total pressure
At what pH is the weak base, pyridine, dissociated by 5%? Pyridine + H2O Pyridium cation + OH- Kb = 1.71*10 ^-9 A. pH = 5.5 B. pH = 6.5 C. pH = 7.5 D. pH = 8.8 E. pH = 10.1
Nitrogen and hydrogen gases react to form ammonia gas. N2(g) + 3 H2(g) 2 NH3(g) At a certain temperature and pressure 1.4 L of N2 reacts with 4.2 L of H2. If all the N2 and H2 are consumed, what volume of NH3, at the same temperature and pressure,..
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The pressure and colume are simultaneously increased so that at every instant P and v are related by the equation, P = Av, where A is a constant.
The zinc content of a 1.45 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc, and then neutralizing excess HCl with NaOH
To what general class of mechanisms does the attack of bromide ion, Br-, on the cyclic bromonium ion
when 0.500 l of a 2.00 m solution of Pb(NO3)2 is mixed with an excess of 1.00m solution of Ki, how many grams lead (II) iodide are formed? ( molar mass: Pb(NO3)2= 331 g;KI 166g; PbI2 =467 g; KNO = 101 g
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This aqueous mixture then reacts with excess aqueous lead (II) nitrate to form 21.75g of solid. Determine the mass percent of sodium chloride in the original mixture?
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