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A 2.00 liter vessel is ?lled with NH3(g) to a pressure of 4.00 atm and the reaction N2(g) + 3 H2(g) ?? 2 NH3(g) comes to equilibrium at a ?xed temperature. At equilibrium it is found that the pressure of H2 is 1.7 atm. What is the equilibrium pressure of NH3? Answer in units of atm.
if 7.o moles of sulfur atoms and 10 moles of oxygen molecules are combined to form the maximum amount of sulfur trioxide, how many moles of which reactant remain unused at the end.
Compute the activation energy for the flashing process. When At 29 o C the average rate is 3.3 flashes every 10 seconds; at 23 degree Celsius the average rate
A compound contain 60.87% carbon, 4.38% hydrogen, and 34.75% oxygen then determine its empirical formula?
Suppose 10.0 g of CH4 is used in a reaction that can theoretically produce 95.8 g of CCl4. What is the percent yield of CCl4 if the reaction produces only 80.0 g of CCl4.
Imagine that you have a 7.00 litre gas tank and a 3.00 litre gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch.
If 12.5 g of magnesium nitride is treated with water, what volume of ammonia gas would be collected at 22°C and 753 mm Hg?
determines how many grams of glucose are in 100 mL of the final solution?
Solving this question helps the student to understand how to find the limiting reactant and how much product is produced and What mass of product may be produced?
Write the expression for the equilibrium constant, Kb, for methylamine also compute the molar concentration of OH- in the 50.0 mL sample of the CH 3 NH 2 solution.
If a 2.1 L reaction vessel initially contains 723 torr of cyclopropane at 485 degrees C , how long will it take for the partial pressure of cylclopropane to drop to below 105 torr ?
Calculate the percent by weight, mole fraction and mole percent of each component in a mixture consisting 9g of water (H2O), 120g acetic acid(CH3COOH) and 115g of ethyl alcohol (C2H5OH).
Determine the partial pressure and total pressure of the gases and Find the partial pressure of carbon dioxide in a gas mixture
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