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If I add 65 grams of calcium chloride to 500 grams of water, what will the boiling
points be of the resulting solution? Kb = 0.512 °C.
A 0.25 moles neon is at 256 mmHg and at temperature of 35°C. What is the volume? (1 atm = 760 mmHg)
𝟐𝑺𝑶𝟐(𝒈) + 𝑶𝟐(𝒈) ⇌ 𝟐𝑺𝑶𝟑(𝒈)
Kc = 6.1 x 104 at 750K. At equilibrium 𝑷𝑺𝑶𝟐 = 𝟏.𝟐𝟐 𝒃𝒂𝒓 and 𝑷𝑶𝟐 = 𝟐.𝟑𝟑 𝒃𝒂𝒓.
Calculate 𝑃 at 750 K (3 points). Hint be sure to convert Kc to Kp first. 𝑆𝑂3
Calculate Kc at 550 K if Δ𝑟𝐻𝑜 = −197.8 𝑘𝐽 𝑚𝑜𝑙−1 (2 points).
Does the decrease in temperature favour products or reactants at equilibrium (1 point)?
what is the molarity for a solution with 25 g mgch in 350 ml water
A=[0.30],[0.60],[0.30] (mol/l)
B=[0.15],[0.30].[0.30] (mol/l)
C= 7.0 x 10-4,2.8 x 10-3,1.4 x 10-3(mol/L-s)
What is the rate equation for the reaction?
The oxyanions IO2- and ClO4- are respectively called:
A canister of butane gas (C4H10, MM=58.12 g/mol) used for portable cooking is available in a store in two sizes, 750 mL and 2.0 L. The 750 mL canister contains 85 g of butane gas with a pressure of 48 atm at 28 C. How many grams of butane gas are present in the bigger canister under the same condition of pressure and temperature?
5. A 0.400 mg initial sample of radioactive iodine–123, used to treat thyroid cancer, decreases to 0.113 mg after 24.0 hrs. Determine the half–life of iodine–123.
- Define oxidation and reduction reactions
- Balance redox reactions using the change in oxidation number method
- Identify the reaction occurring in the different parts of the cell
- Define reduction potential, oxidation potential, and cell potential
- Calculate the standard cell potential
- Relate the value of the cell potential to the feasibility of using the cell to generate an electric current
- Describe the electrochemistry involved in some common batteries:
a. Leclanche dry cell
b. Button batteries
c. Fuel cells
d. Lead storage battery
- Apply electrochemical principles to explain corrosion Explain the electrode reactions during electrolysis Describe the reactions in some commercial electrolytic processes
How many liters of 0.55 M HCl is required to neutralize 1.10 g of sodium carbonate
(Na2CO3)? (molar mass of Na2CO3 = 105.99 g/mol)
2HCl + Na2CO3 → 2NaCl + H2CO3
