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Calculate DeltaHrxn for the following reaction: CH4(g) + 2Cl2 (g) --- CH2Cl2(g) + 2HCl(g) Use the following reactions and given delta H's: CH4(g) + Cl2 (g) --- CH3Cl+HCl(g) Delta H = -99.6kJ CH3Cl(g) + Cl2 (g) --- CH2Cl2+HCl(g) Delta H = -105.8kJ
The density of a sodium sulfate solution is 1.07 g/cm3. The solution is 8.00% sodium sulfate by mass. How many cm3 of the solution are needed to supply 4.28 g of sodium sulfate?
how many grams of Mg(OH)2 will be needed to neutralize 25ml of stomach acid if stomach acid is .10M HCL
Marble (calcium carbonate) reacts with hydrochloric acid solution to form calcium chloride solution, water, and carbon dioxide. What is the percent yield of carbon dioxide
What is the molar concentration of a H3PO3 solution if 150.00 mL of the solution was required to neutralize 75.00 mL of NaOH whose concentration was 1.50 molar?
A 15.0--mL unknown sample of aqueous acetic acid, CH3COOH(aq), was titrated using 0.800 M NaOH. If the titration endpoint was found to be 20.0 mL.
A 25.0g sample of nitrogen (N2) has a volume of 50.0L and a pressure of 630.0 mmHg. What is the temperature of the gas.
Consider 2 Al + 6 HCl → 2 AlCl3 + 3 H2 , the reaction of Al with HCl to produce hydrogen gas. This reaction has a yield of 82.5 percent. How much HCl are needed to produce 14.0 L of H2 at 351 K and 1.11 atm
For 550.0 mL of pure water, calculate the initial pH and the final pH after adding 0.010 mol of pH
the volumetric flask during weighing by difference after recording the mass, how would it affect the final result for his calculated molecular mass of the metal carbonate?
What is the pH of the solution if [OH-] of an ammonia solution is 1.0 X 10-2M?
A gaseous mixture of Oxygen(O2 )and Nitrogen(N2 )contains 40.8 grams N2(nitrogen) by mass then determine what is the partial pressure of O2(oxygen) in the mixture if the total pressure is given= 345 mmHg.
Solution A is 2.00 L of a 2.00 M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00 M aqueous solution of potassium hydroxide. React the two solutions. Determine the concentrations of all ions left in solution (from part a) and..
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