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Problem- The absorbance of an ionic aqueous solution is 0.301. What is the ratio of intensities of the passed light over the incident light for that solution?
Solve the above problem and provide steps with explanation
the acid-dissociation constant for hypochlorous acid hclo is 3.0 x 10- 8. calculate the concentration of h3o at
4 C3H5O9N3(l) → 12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g) If a sample containing 2.01 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how many total moles of gas are produced?
Write out all equations (but you do not have to do the integration!) how you would calculate the absolute entropy of Cl2(g) at 298K. For full credit, you must include the limits of integration.
Each student recorded the temperature change and calculated the enthalpy of neutralization. Identify the student who observes a temperature change that will be different from that observed by the other two chemists. Explain why and how (higher or ..
Calculate the pH after the following additions of the KOH solution (a) 10.0 mL (b) 11.5 mL (c) 15.0 mL (the Ka for CH3COOH = 1.8 x 10^-5)
Draw the structures of ALL of the diferent alkenes produced from an E2 elimination on 2-bromo-3,4-dimethylpentane.
A 100 L reaction container is charged with 0.704 mol of NOBr, which decomposes at a certain temperature say between 100 and 150ºC according to the following reaction
Electrochemistry has a wide range of applications. Research and describe one job, outside the field of chemistry, that uses electrochemical knowledge
For the reaction Na2CO3(aq)+2HCl(aq)= 2NaCl(aq)+CO2(g)+H2O(l), suppose you have 100 mL of 3.80M Na2CO3. How many milliliters of 0.920 M HCl would you have to add to the sodium to consume the Na2CO3 completely
Calculate the number of grams of carbon monoxide produced from the detonation of 200.0g of TNT (C7H5N3O6) given the following reaction
Arrange the following solutions in order of decreasing freezing point: 0.20 m Fe(OH)2, 0.15 m C6H12O6, 0.10 m K3PO4, 0.15 m CH3CH2COOH, 0.35 m LiI.
Assume constant temperature and the reaction goes to completion, producing as much nitrogen dioxide (NO2) as possible according to the following equation. What is the total pressure, in atm, in the system after the reaction?
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