5)
Salt is ionic in nature.
They will dissolve in polar solvent.
They will not dissolve in non polar solvent.
Answer: No
6)
Molar mass of NO,
MM = 1*MM(N) + 1*MM(O)
= 1*14.01 + 1*16.0
= 30.01 g/mol
mass of NO = 90 g
mol of NO = (mass)/(molar mass)
= 90/30.01
= 2.999 mol
According to balanced equation
mol of NH3 formed = moles of NO
= 2.999 mol
Molar mass of NH3,
MM = 1*MM(N) + 3*MM(H)
= 1*14.01 + 3*1.008
= 17.034 g/mol
mass of NH3 = number of mol * molar mass
= 2.999*17.03
= 51.1 g
According to balanced equation
mol of H2O formed = moles of NO
= 2.999 mol
Molar mass of H2O,
MM = 2*MM(H) + 1*MM(O)
= 2*1.008 + 1*16.0
= 18.016 g/mol
mass of H2O = number of mol * molar mass
= 2.999*18.02
= 54.0 g
Answer:
Mass of NH3 = 51.1 g
mass of H2O = 54.0 g
Only 1 question at a time please
5. Will a salt dissolve in a nonpolar solvent? 6. Ammonia NH3, can be synthesized by...
1. What is the mass percent of oxygen in H202? 2. What would happen if you added more solute to a saturated solution? 3. What would happen if you added more solute to an unsaturated solution? 4. Will a polar solute compound dissolve in a nonpolar solvent? 5. Will a salt dissolve in a nonpolar solvent? 6. Ammonia NH3, can be synthesized by the following reaction: 2NO+ 5H2 + 2NH3 +2 H2O If you start with 90.0 grams of NO...
Review: 1. Ammonia NH,, can be synthesized by the following reaction: 2NO 5H 2NH,+ 2H,0 what is the theoretical yield If you start with 90.0 grams of NO and an unlimited supply of H of ammonia, in grams? a. How much water is produced? b. What is the percent yield if 25 grams of ammonia are produced? C. 10X
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Ammonia can be synthesized by the reaction: 3 H2 (g) + N2 (g) → 2 NH3(g) What is the theoretical yield of ammonia, in Kg, that we can synthesize from 5.22 Kg of H2 and 31.5 Kg of N2? If we have 20 kg of NH3 fine the percent yield.
Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows: 2NH3(aq)+CO2(aq)→CH4N2O(aq)+H2O(l). In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the theoretical yield of urea, limiting reactant, and percent yield for the reaction.
Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows: 2NH3(aq)+CO2(aq)→CH4N2O(aq)+H2O(l) In an industrial synthesis of urea, a chemist combines 141.3 kg of ammonia with 211.4 kg of carbon dioxide and obtains 166.4 kg of urea. Determine the theoretical yield of urea Determine the percent yield for the reaction.
Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows: 2NH3(aq)+CO2(aq)→CH4N2O(aq)+H2O(l) In an industrial synthesis of urea, a chemist combines 128.2 kg of ammonia with 211.4 kg of carbon dioxide and obtains 170.7 kg of urea. B. Determine the theoretical yield of urea C. Determine the percent yield for the reaction.
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the percent yield of the reaction
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