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The system H2 (g) + I2 (g) ?? 2 HI(g) is at equilibrium at a ?xed temperature with a partial pressure of H2 of 0.200 atm, a partial pressure of I2 of 0.200 atm, and a partial pressure of HI of 0.100 atm. An additional 0.15 atm pressure of HI is admitted to the container, and it is allowed to come to equilibrium again. What is the new partial pressure of HI?
Determine How much sodium hydroxide (in grams) is required to form 546 mL of solution with a pH of 10.00?
Determining the limiting reactant and mass of the product - which reactant is the limiting reactant? What mass of product may be produced?
Iincreasing the total pressure on the system by decreasing its volume, (c) adding gaseous I2 to the reaction mixture?
How much heat (in kJ) is evolved in converting 1.20 mol of steam at 134.0°C to ice at -55.0°C.
A buffer (pH 3.70) was prepared by mixing 1.00 mole of formic acid and 1.00 mole of sodium formate to form an aqueous solution with a total volume of 1.00 L.
A reaction initially contains 0.1 moles of H2(g) and I2(g) in a 1L flask. At equilibrium the final concentration of HI(g) is 0.19M. What is Kp for this reaction.
What is the molarity of a solution that contains 41.0 g of vitamin B1 hydrochloride (molar mass = 337 g/mol}) in 280 mL of solution?
Determine value for the rate of formation of HCl during the same interval of 3 seconds If the rate of disappearance H2 = -0.13 M/s at this specific time?
Determine the percent yield if An 8.50 grams sample of Ammonia gives 12.0 g of Nitric Oxide?
A nonelectrolyte solution adsorbs on an electrically neutral solid through a liquid. Two surfaces of this type are brought close to one another in the liquid such that they interact.
Calculate the molar concentration of OH - ions in an 1.43 M solution of hypobromite ion, BrO- (Kb = 4.0 10-6).
calculate (a)molality? (b)molarity of NaCl? (c) What is the mass/mass and remove the most loosely held e- from a gaseous atom in a ground state
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