10. In an experiment, a sample was 90% decomposed in 24 min. Approximately how long would this decomposition have taken if the sample had been heated 20°C higher? (Hint: Assume the rate doubles for each 10°C rise in temperature.)

11. Find which kind of catalyst is necessary to facilitate the reaction between molecular nitrogen and molecular hydrogen to make ammonia (several words description)

Calculate the pH when 54.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

Predict how the equilibrium will shift (to the left, to the right or no change) with each of the following stresses: a. 2H2 (g) + 2NO (g) → N2 (g) + 2H2O (g) i. Increase [H2] ii. Decrease [NO] iii. Decrease the pressure (by increasing the volume) b. CO (g) + 1/2O2 (g) → CO2 (g) + 283 kJ i. Decrease temperature ii. Increase pressure (by adding He (g)) c. H2O (l) → H + (aq) + OH− (aq) i. Add NaOH d. 4NH3 + 5O2 (g) → 4NO (g) + 6H2O (g) + energy i. Increase temperature ii. Remove NO (g) e. Fe3O4 (s) + 4H2 (g) ↔ 3Fe (s) + 4H2O (g) i. adding more H2 to the mixture ii. adding more Fe (s) iii. removing H2 iv. adding a catalyst

What would be the difference in reactivity if ethyl 3-methylbenzoate was treated in a reduction with NaBH4 vs LiAlH4? I know that NaBH4 is only powerful enough to reduce ketones and aldehydes, and ethyl 3-methylbenzoate has a ketone group, but I am confused as to how different LAH would be?

1) How many grams of solid potassium cyanide should be added to 1.50 L of a 0.236 M hydrocyanic acid solution to prepare a buffer with a pH of 10.287 ?

grams potassium cyanide = ______g.

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2) The volume of water needed to dissolve 0.0661 grams of lead fluoride is _____ L.

Assume no volume change upon addition of the solid.

You need 700. mL of a 5.0 % (m/v) glucose solution. If you have a 29 % (m/v) glucose solution on hand, how many milliliters of this solution do you need?

Calculate the theoretical amounts of 0.1000 M NaOH titrant used to titrate 0.8 and 0.9 g KHP. please show work!

Use the Henderson-Hasselbalch equation to calculate the pH of each solution:

a) a solution that is 0.170M in HC2H3O2 and 0.125M in KC2H3O2

Express your answer using two decimal places.

b) a solution that is 0.200M in CH3NH2 and 0.125M in CH3NH3Br

Express your answer using two decimal places.

Cyclohexanol is converted to cyclohexanone using hypochlorous acid. Excess hypochlorous acid is removed by adding sodium bisulfite. The aqueous reaction mixture is then saturated with sodium chloride and placed in a separatory funnel with methylene chloride (dichloromethane). Refer to the density table found here if needed. The boxes in the diagram represent the layers of the separatory funnel. Place the labels in the appropriate box.

How "wastage reactions" can be minimized by taking into account such factors

1) radical stability, 2) radical 1/2 life, 3) monomer reactivity?

Which of the following is a redox reaction? More than one answer may be correct.

HBr(aq) + KOH(aq) → H2O(l) + KBr(aq) SO3(g) + H2O(l) → H2SO4(aq)

HBr(aq) + Na2S(aq) → NaBr(aq) + H2S(g)

NH4+(aq) + 2 O2(g) → H2O(l) + NO3–(aq) + 2 H+(aq)

2 Na(s) + Cl2(g) → 2 NaCl(s)

None of the above are redox reactions.

Some free radical chemical reactions start with the photodissociation of I2 molecules into Iodine atoms (gas phase) by light with a wavelength shorter than about 792nm. A 100.0mL glass tube, pressure= 55.7mtorr and temperature 25.0C contains I2 molecules What minimum amount of energy must be absorbed by the iodine in the tube to dissociate 15% of the the molecules?

What means charge based separation method in analytical chemistry?