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Write the balanced equation for the ionization of the weak base pyridine, C5H5N, in water, H2O. Phases, such as (aq) or (l), are optional.
Write the equilibrium constant expression, Kc , for the following chemical reaction.
The rate law of a given reaction is rate=k[reactant]^2, with k=2.64 x 10^-4 M-1min-1. If the initial concentration is 0.0250 M, what is the initial rate?
Determine the maximum amount of P4S10(444.545 g/mol) that can be produced from 18.27 grams of Phosphorous (123.895 g/mol) and 9.42 g of sulphur (256.52 g/mol)
Calculate the concentration of the acetate ion (mol/L) in a solution prepared by dissolving 1.00×10-2 mol of HCl(g) in 1.00 L of 9.00×10-1 M aqueous acetic acid. Equilibrium constants may be found in an appendix to your text.
Pressure is gradually decreased from 87.7mL to 42.6mL. What is the final pressure of ammonia if there is no change in pressure?
In a chemical reaction (unbalanced equation), AsF3 + C2Cl6 -> AsCl3 + C2Cl2F4, the theoretical yield of C2Cl2F4 was calculated to be 1.86 mol. If the percent yield in the reaction was 77.2%,
Write the structural formula for each of the following compounds. 3-ethyl-2,3-dimethylpentane
whole bunch of different PE diagrams and I'm asked which one is the highest temperature dependent and which one is the lowest
Calculate the hydronium ion concentration and the pH after the addition of 0.25 mL of 0.10 M HCl to each one.
If 5.85mL of 0.1000 M NaOH solution is needed to just neutralize excess acid after 20.00 mL of HCl was added to 1.00 g of an antacid, how many moles of acid can the antacid counteract per gram?
How many gm of dry NH4Cl need to be combined to 2.30L of a 0.300M solution of NH3, to prepare a buffer solution of pH 8.85.
The magnesium and calcium ions present in seawater([Mg2+] = 0.059 M and [Ca2+] = 0.011 M) can be separated by selective precipitation with KOH.
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