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Ammonia gas is dried using
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Explain why ammonia gas cannot be dried with concertrated hydrochloric acid during it's preparation in the laboratory.
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Concentrated HCl means to me a solution of HCl. A solution means water so there can't much drying
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To find the mass of the ammonia gas, we can use the Ideal Gas Law equation: PV = nRT. Rearranging this equation gives us n =
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To find the mass of the ammonia gas, we need to know the values for pressure (P), volume (V),
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At 65C,a sample of ammonia gas exerts a pressure of 10.2 atm..Calculate the pressure when the volume of gas is reduced to one
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To solve this problem, we can use Boyle's Law, which states that the pressure and volume of an ideal
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Ammonia is often produced by reacting nitrogen gas with hydrogen gas.
How many liters of ammonia gas can be formed from 12.9 L of
Top answer:
balance the equation: 3H2+N2>>2NH3 so you get 2/3 of the moles of Hydrogen gas.. moles H2=PV/RT
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QUESTION 11
Ammonia gas is formed from nitrogen gas and hydrogen gas, according to the following equation: N2 (g) + 3H2 (g)
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83.3
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9. The reaction of 50 mL of N2 gas with 150 mL H2 gas to form ammonia via the equation: N 2(g) + 3H2 (g) → 2NH3 (g) will
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Well, let's do a little math here. According to the balanced equation, for every 1 mole of N2 gas,
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Ammonia, NH3, is widely used as a fertilizer and in many household cleaners. How many moles of ammonia are produced when 6 mol
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N2 + 3H2 ==> 2NH3 The equation tell you that you get 2 mols NH3 for every 3 mols H2 so if you have 6
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in an experiment, ammonia gas, NH3(g) was bubbled through distilled water. Some of the dissolved ammonia gas, NH3, reacted with
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c) NH3 + HOH ==> NH4^+ + OH^- A. The answers depend upon which acid/base theory used. I'll assume
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a mass of 80 grams of hydrogen gas is heated with nitrogen gas to produce ammonia gas .what is the mass of ammonia that will be
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H2 is 2 grams/mol so we have 40 mols of H2 which is 80 mols of H for each mol of H we get 1/3 mol of
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A commercial refrigerator unit accidentally releases 12.5 L of ammonia gas at SATP. Determine the mass and number of molecules
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Better check your formulas 1 mole of gas at STP occupies 22.4L So, you have 12.5/22.4 * 6.023*10^23
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