Solution - first see balance reaction of formation of hydrazine -
2NaOH + Cl2 +
2NH3
N2H4 + 2NaCl + 2H2O
a)
From balance reaction it is clear that one mole of chlorine gas required two moles of NaOH , were NH3 is in excess, so we have to check moles of NaOH and chlorine only.
# Molar mass of NaOH = 40 g/mol
# Molar mass of chlorine gas = 70.9 g/mol
#Molar mass of hydrazine = 32.04 g/mol
#mass of NaOH = 25 .0 g
#mass of chlorine gas = 30.0 g
Now we can calculate number of moles by using molar mass and mass of individual component.
Number of moles (n) = (mass of NaOH /Molar mass of NaOH)
= (25.0 g /40.0 g / mol )
=0.625 mol of NaOH
Now we have to calculate number of moles of chlorine gas =(mass of chlorine gas /molar mass of chlorine gas)
=(30.0 g /70.9 g/mol)
= 0.4231 mol of chlorine gas
But from balance reaction it is clear that one mole of chlorine gas required two moles of NaOH, so theoretically moles require for complete reaction = (moles of chlorine gas x 2)
= (0.4231 mol x 2)
= 0.8462 mol of NaOH required but we
have only 0.625 mol, so limiting reagent is NaOH ( 0.8462 mol
(theoretical moles)
0.625 mol)
Now we have to calculate theoretical yield of hydrazine against limiting moles of NaOH ,
Theoretical yield of hydrazine = ( moles of NaOH x molar mass of hydrazine)
= (0.625 mol x 32.04 g/mol )
= 20.0 g
b)
Amount of hydrazine recovered ( practical yield) = 8.00 g, what is percentage yield?
We know that,
percentage yield = (practical yield /Theoretical yield) x 100
= (8.00 /20.0 )x100
= 40%
In the Raschig Process, ammonia, NH3, is oxidized with sodium hypochlorite (formed from NaOH and Cl2)...
Cl2 + 3F2 → 2CIF: Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 500g of chlorine and 95.0g of fluorine. a) What is the limiting reagent? b) What is the theoretical yield of chlorine trifluoride in grams? c) How many grams of excess reactant remain un-reacted? 2C2H2 + 50, 400, + 2H2O Oxyacetylene torches used in welding and cutting steel reach temperatures near 2000'C. The reaction involved is the complete combustion of acetylene (CH2). Starting with...
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
Limiting Reactants, Excess Reactant, and % Yield Name H2+Cl2HCI A gaseous mixture containing 7.5 g of H; gas and 9.00 g of Cl2 gas react to form hydrogen chloride gas. а) Which is the limiting reactant? If all the limiting reactant is consumed, how many grams of HCl are produced? How many grams of excess reactant remain un-reacted? b) c) Cl2+3F22CIF Chlorine reacts with fluorine to form gaseous chlorine trifluoride. You start with 50.0g of chlorine and 95.0g of fluorine....
Name FUL L U Stoichiometry worksheet (Lab) Please complete the following problems during lab. Do all of your work on a separate sheet of paper. Show all of your work for full credit and circle your final answer. 1) How many moles of CO2 are produced when 2.5 moles of O2 react according to the following equation? C3H8 (8) +502 (8) ► 3002 (8) + 4H20 (8) 2) In the reaction 2 C(s) + O2(g) 66.0 g of carbon monoxide?...
Nitrogen gas can be prepared by passing gaseous ammonia over solid CuO at high temperatures. The other products of the reation are solid copper and water vapor. If a sample containing 18.1g of NH3 is reacted with 90.4g of CuO, which is the limiting reactant? How many grams of N2 will be formed? What is the theoretical yield ? If 6.63g are actually producted what is the percent yield in this case? I believe the balanced equation is: 2NH3(g) +...
When carboxylic acid is mixed with aqueous ammonia solution, ammonium carbonate is formed: H2CO3 (aq) + 2 NH3 (aq) → (NH4)2CO3(aq) a. If 10.00 mL of a 0.105 M NH3 solution reacted with 25.00 mL of a 0.0835 M H2CO3 solution, which reactant is the limiting reagent? (6 pts) b. What is the maximum number of moles of ammonium carbonate that can be formed? (3 pts) c. What is the molarity of the ammonium carbonate solution given that the two...
How many grams of sodium iodide are required to react completely with 3.01 x 1023 molecules of chlorine? 2 NaI + Cl2 ------> I2 + 2 NaCl A. 1.50 g B. 37.5 g C. 150. g D. 74.9 g 1 points QUESTION 2 When 22.0 g of NaOH and 21.0 g of H2SO4 are mixed and react according to the reaction: 2 NaOH + H2SO4 ------> Na2SO4 + 2 H2O, which is the limiting reagent? A. NaOH B. H2SO4 C....
cal 22) Given that 4 NH3 5 O2-4 NO+6 HyO, if 3.00 mol NH3 were made to react with excess of 22) Oxygen gas, the amount of H2O formed would be A) 4.50 mol. B) 2.00 mol. C) 6.00 mol. D) 3.00 mol. E) none of the above 23) Which of the following statements is FALSE? A) The actual yield is the amount of product actually produced by a chemical reaction. B) The percent yield- 23) Actual Yield Theoretical Yield...
Chlorine gas reacts with phosphorus to produce phosphorus pentachloride as shown in the chemical equation below. What is the maximum number of grams of PCls are produced from 3.5 g of Cl2 and excess P? 5C12(g) + 2P(s) → 2PC13(s) 2) What is the theoretical yield of chromium that can be produced by the reaction of 40.0 g of Cr2O3 with 8.00 g of aluminum according to the unbalanced chemical equation below? Al(s) + Cr2O3(s) → Al2O3(s) + Cr(s) Ammonia...
22) Given that 4 NH3 +50,-- 4 NO:6 HO.if 3.00 mol NHy were made to react with excess of oxygen gas, the amount of H2O formed would be: A) 4.50 mol B) 2.00 mol. C) 6.00 mol. D) 3.00 mol. E) none of the above 23) Which of the following statements is FALSE? A) The actual yield is the amount of product actually produced by a chemical reaction. B) The percent yield - Actual Yield Theoretical Yield"100 C) The limiting...