Learn more about our help with Assignments: Chemistry
Search & Filtering
Using the overall reaction for making synthetic gypsum by means of recycling sulfur dioxide gas:
SO2(g) + CaSO3(s) + 1⁄2O2(g) + 2 H2O(l) ˇ CaSO4 . 2H2O(s) + CO2(g)
(a) determine the mass of synthetic gypsum produced for every kilogram of sulfur dioxide recycled.
(b) determine both the mass and the volume of water required to recycle a kilogram of sulfur dioxide.
SO2(g) + CaSO3(s) + 1⁄2O2(g) + 2 H2O(l) ˇ CaSO4 . 2H2O(s) + CO2(g)
(a) determine the mass of synthetic gypsum produced for every kilogram of sulfur dioxide recycled.
(b) determine both the mass and the volume of water required to recycle a kilogram of sulfur dioxide.
Can you explain how to write chemical formulas?
If 35.5g of ion was made to react with chlorine the mass of the product obtained would be either 80.1g or 103.01g depending on the amount of chlorine present.Which gravimetric ion will be in accordance?
A salt solution containing ferrous ion was titrated with (9.80000x10^-3) M KMnO4 solution. The mean of 3 acceptable, corrected titration values was (1.400x10^1) mL. Calculate the moles of ferrous ion reacting in each titration portion.
a) A student places 289 g of water in a calorimeter at 14.9° C. She then drops in a piece of silver at 87.5 degrees C. If the final temperature of the water is 19.7°C, what is the mass of the silver? (cAg = 0.0558 cal/g°C)
b) Later, her lab partner pours 200.6 g of water at 95.8°C into a 300.9 g silver bowl at 18.4°C. What will the final temperature be (assuming that no heat is transferred to or from the environment)?(algebra first)
c) Realizing that her prior experiment was imperfect, the first student decides to find the heat capacity of the calorimeter. She places 165 g of water at 18.5°C in a calorimeter. She then adds 85 g of water at 84.7°C. If the final temperature of the system is 39.5°C, what is the heat capacity of the calorimeter?
d) Her partner then places 285.5 g of water at 91.6°C and puts it in the calorimeter. He then drops in 16.5 g of ice at -3.5°C.What will the final temperature of the system be? ( HΔ fus of ice = 79.7 cal/g, c of ice = 0.50 cal/g°C)
b) Later, her lab partner pours 200.6 g of water at 95.8°C into a 300.9 g silver bowl at 18.4°C. What will the final temperature be (assuming that no heat is transferred to or from the environment)?(algebra first)
c) Realizing that her prior experiment was imperfect, the first student decides to find the heat capacity of the calorimeter. She places 165 g of water at 18.5°C in a calorimeter. She then adds 85 g of water at 84.7°C. If the final temperature of the system is 39.5°C, what is the heat capacity of the calorimeter?
d) Her partner then places 285.5 g of water at 91.6°C and puts it in the calorimeter. He then drops in 16.5 g of ice at -3.5°C.What will the final temperature of the system be? ( HΔ fus of ice = 79.7 cal/g, c of ice = 0.50 cal/g°C)
Calculate the number of mole presents in certain mass of gas occupying 6.5dm3 at atm and 15•C. ( R=0.082 atm dm3 K-1 mole-1).
Describe the structure and function of nuclear envelope.
Explain in brief the regulation of glycogen metabolism.
Compare the energetics of metabolic oxidation of glucose and a fatty acid.
Explain the mechanism of action of the enzyme aconitase on citrate in TCA cycle.
