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what will the final mixture contain if 14.0 g of N2 and 35.5 g of Cl2 react to completion and the balanced equation is: N2+3Cl2--->2NCl3
What is the percentage yield if 465 grams of hydrogen reacted with excess nitrogen and 455 grams of ammonia is formed N2 (g) + 3 H2 (g) 2NH3(g)
An aqueous solution contains 4.90% NH3 (ammonia) by mass. The density of the aqueous ammonia is 0.979 g/mL. What is the molarity of NH3 in the solution?
how many grams of sodium acetate must be added to 1.00 L of a .200 M acetic acid solution to form a buffer of 4.20? Ka value for acetic acid is 1.8x10^-5.
determine the heat released when (ethene) CH2 CH2 reacts with hydrogen gas and form CH3CH3.If Bond enthalpies given are H H : 436 kJ/mol,C Br : 276 kJ/mol,C C : 612 kJ/mol,C C : 348 kJ/mol,C H : 412 kJ/mol;
What is the emprical formulae of the compound whose composition by mass is 1.32g of carbon dioxide contain 0.36g of carbon.
A 0.456 gram sample of an unknown monoprotic acid (let's call it HZ) was dissolved in some water (you pick the amount). Then the acidic solution was titrated to the equivalence point with 32.5 mL of 0.174 M KOH.
How many kilograms of chalcopyrite must be mined to obtain 290. g of pure Cu ?
For alloys of two hypothetical metals A and B. Find out composition of phase boundary (or solubility limit) for both and phases at this temperature.
A mixture of gases contains 0.290 mol CH4, 0.250 mol C2H6, and 0.270 mol C3H8. The total pressure is 1.60 atm. Calculate the partial pressure of the gases.
53.5 g of an ideal gas of molecular weight = 30.5 g/mol are confined at a pressure of 133 mmHg. The density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.
how many liters of 13.5 molar HCl stock solution are needed to make 10.5 liters of a 1.8 molar HCl solution?
4 C3H5O9N3(l) → 12 CO2(g) + 6 N2(g) + O2(g) + 10 H2O(g) If a sample containing 2.01 mL of nitroglycerine (density = 1.592 g/mL) is detonated, how many total moles of gas are produced?
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