Physical Chemistry Answers

After being poured into a pan, 10.0 moles of water were heated on an electric stove. During this time, the temperature of the liquid rose from 26 ℃ to 38 ℃. How much heat, in J, was absorbed by the water? Use c = 73.32 J/mol K.

After being poured into a pan, 10.0 moles of water were heated on an electric stove. During this time, the temperature of the liquid rose from 26 ℃ to 38 ℃. How much heat, in J, was absorbed by the water? Use c = 73.32 J/mol K.

During an experiment to find the enthalpy change for the reaction between zinc and copper sulfate solution a student recorded the temperature of the copper sulfate solution for two minutes. She then added the zinc and continued to record the temperature whilst stirring the solution in the 'coffee cup' calorimeter. She plotted a graph of her data. What value should she use for ΔT when calculating her result?

Cisplatin or Platinol has a chemical PtCl2(NH3)2 that is used in the treatment of certain cancers. Calculate (a) the amount (mol) of compound in 285.3 g of cisplatin; (b) the number of hydrogen atoms in 0.98 mol of cisplatin.

Solution #1 is a 0.025 M solution of hypochlorous acid, HOCl (Ka = 3.0 × 10–8). Calculate each of the

following quantities for Solution #1.

(a) [H+] in Solution #1

Bituminous coal is a type of coal that is composed of carbon with small amounts of hydrogen, oxygen, nitrogen, and sulfur. The formula for a sample of bituminous coal is 

C137H97O9NS. Calculate the amount of carbon in 65.0 kg of the sample.

3 grams of Aluminum are reacted with 4 grams of Copper (II) sulfate to produce Aluminum sulfate

and the metal copper.

a) Which is the limiting agent?

b) How many grams of copper are formed

How many grams of CO2 are produced when 100 g C4H10 undergoes combustion with 200 g O2?

Use the following molar masses: C4H10=58g/mol, O2=32 g/mol and CO2=44g/mol.

Compare the moles of product formed from each reactant.

Using the "equipartion" of energy concept, estimate the ideal gas $c_p$ (not $c_v$) in units of $k_B$ for "low-temperature" where no vibrational modes are activated. (if you calculate $c_p = 42k_B$, enter 42 as your answer)

The equilibrium constant for the autoprotolysis of water, H2O (l) H+(aq) + OH−(aq), is Kw =

[H+][OH−] = 1.008 × 10−14 at 298 K. After a temperature-jump, the reaction returns to

equilibrium with a relaxation time of 3.7 x 10-5 s at 298 K and pH ≈ 7. Given that the forward

reaction is first-order and the reverse is second order overall, calculate the rate constants for the forward and reverse reactions.