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The zinc content of a 1.45 g ore sample was determined by dissolving the ore in HCl, which reacts with the zinc, and then neutralizing excess HCl with NaOH. The reaction of HCl with Zn is shown below:Zn+2HCL--ZnCl2+H2
The ore was dissolved in 150 mL of 0.600 M HCl, and the resulting solution was diluted to a total volume of 300 mL. A 20.0 mL aliquot of the final solution required 8.48 mL of 0.508 M NaOH for the HCl present to be neutralized. What is the mass percentage (%w/w) of Zn in the ore sample?
How do you calculate the pH of a solution given the concentration of OH- ions?
According to the following reaction, how many grams of carbon tetrachloride are required for the complete reaction of 21.1 grams of methane (CH4)?
Celsius and heated to the temperature of 275 degree Celsius at a constant pressure of 0.975 atm. compute the work done?
Lucite is 71.4% carbon, 9.59% hydrogen, and 19.01% oxygen. What is the empirical formula for Lucite?
A test solution contained 2 mL of 0.10 M Ag+. A silver strip was dipped into the test solution, and a cell potential of 0.0592 V was measured against an Ag/Ag+(1.0M) reference half-cell.
Explain the type of nonrenewable energy resource used and their short-term and long-term effects on the environment
If a mixture of 35.8 g of CH4 and 75.5 g of S reacts, how many grams of H2S are produced? CH4(g)+4S(g)-->CS2(g)+2H2S(g).
Calculate the standard enthalphy change for the following reaction.
Hydrogen is produced when methane(CH4) reacts with water. The other product is CO2. Using 80.0g of methane and 16.3g of water, how many liters of H2 can be produced at STP? what is the limiting reactant?
Show by explicit integration that the 1s and 3s wave functions of the hydrogen atom are orthogonal. Note that in integrals over r
1 mole of a hydrocarbon of formula CnH2n was burned completely in oxygen producing carbon dioxide and water vapour only. It required 192 g of oxygen. Work out the formula of the hydrocarbon.
A first order reaction has a rate constant of 0.342 sec^-1 at 29.5 degrees C. If the activation energy is 69 kJ, calculate the temperature in degrees C at which the rate constant is 0.428 sec^-1.
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