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The total quantity of coal burned in Canada and the United States in a year is approximately 450 x 106 t. The average quantity of sulphur in coal is 2.5%.
a) Calculate the mass of sulphur contained in coal.
b) Calculate the mass of calcium carbonate required to eliminate sulphur (IV) oxide. (You may assume that 1 mole of sulphur will produce 1 mole of sulphur (IV) oxide.) 5 marks
c) Give your comments on problems related to this method of reducing pollution. (You may find it useful to know that a railcar of calcium sulphite weighs approximately 100 t.)
d) Have you any other suggestion on how to fight acid rain caused by coal combustion?
allowed to expand adiabatically against constant Pext = 10 atm. Compute the final T, ?U, and ?H for this process. Use Cv = 20.8 J/mol*K and assume the gas is ideal.
A 115 mL sample of a 11.0 M ethylene glycol (rm C_2H_6O_2) solution is diluted to 1.40 L.What is the freezing point of the final solution? (Assume a density of 1.06 g/mL for the final solution.)
however, it takes more CaCl2 to form a White solid in one of the solutions than the other. Using the data from your experiment to help, explain what is happening when CaCl2 is reacted with the NaHCO3 (aq) or Na2CO3 (aq) solutions.
completely neutralize 50.00 ml of a weak monoprotic acid, HA. when 32.64 ml of NaOH are added to another 50.00 ml of the acid, the pH reading was 4.80. Calculate Ka for the acid using the partial neutralization method.
17.5 kj of heat is required to melt 52.5g of ice at its melting point. How much heat is required to raise the temperature of 52.5g of water from its melting point to its boiling point. express answer in kj.
A gas bottle contains .65 mol of gas at 730 Hg pressure. If the final pressure is 1.15 atm, how many moles of gas were added to the bottle?
The antifreeze in a car was a 50% by weight solution of ethylene glycol C2H6O2 in water. Calculate the boiling point and freezing point of this solution. (for H2O: Kb= 0.52 C/m... Kf=1.86 C/m
Estimate the temperature where ?G=0 for the following reaction: (giving ?H= -176 kJ, and ?S= -284.5 J/K) CAUTION Beware of units. NH3(g)+HCl(g)--->NH4Cl(s)
A solution contains .229 M sodium acetate and .157 M acetic acid. What is the pH of this solution. How is Ka calculated
Calculate the theoretical yield in grams of methyl piperate from 3.6g of C9H17O5P and using 5% of molar excess of piperonal.
The water level in a graduated cylinder initially at 223 mL rises to 282 mL after a piece of lead is submerged. What is the mass in grams of the lead?
The stock solution is 500 ?g/mL and you want to obtain a final concentration of 1?M. What volume of the stock solution do you need to make 10 milliliters of the 1 ?M solution? Also: What is the molar mass of PMA?
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