FL WO-I) Determine the limiting reactant (L.R), the mae in grams gas that could be formed...
35 and 36 thank you
QUESTION 35 Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N204 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N204 = 92.02 g/mol, N2H4 = 32.05 g/mol. N204(0) + 2 N2H40 →3N2(g) + 4H2O(9) O LR = N2H4, 59.0 g N2 formed O No LR, 45.0 g N2 formed O LR = N2H4, 13.3 g N2 formed O LR =...
mttps://www.o... Student Cons... Diagnostic Re... Quiz: E D Question 55 1 pts Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N204 and 45.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N H4 = 32.05 g/mol. N2O4(1) + 2 N2H4(1) 3 N2(g) + 4H2O(g) OLR-N2H4, 59.0 g N formed OLR-N204, 105 g Ny formed No LR, 45.0 g N2formed OLR-N2H4, 13.3 g N...
Determine the limiting reactant for the reaction of 50.0 g N204 and 50.0 g N2H4. Some possibly useful molar masses are as follows: N204 = 92.02 g/mol, N2H4 = 32.05 g/mol. N2016) + 2N2H4() — 3 N2(g) + 4H2O(g) ON2 O N₂ Ha N20 ОНО
Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 50.0 g N 2O 4 and 45.0 g N 2H 4. Some possibly useful molar masses are as follows: N 2O 4 = 92.02 g/mol, N 2H 4 = 32.05 g/mol. N 2O 4( l) + 2 N 2H 4( l) → 3 N 2( g) + 4 H 2O( g) LR = N2O4, 45.7 g N2 formed LR = N2O4, 105 g...
Extra Credit (7 pts each) SHOW WORK! 1) When a solution of Magnesium Chloride and Silver Nitrate are mixed: a) Write and balance the chemical reaction. Include all phases of both reactants and products. b) Write the complete ionic and net ionic equations for the reaction. c) Identify what kind of reaction is occurring. 2) Given the following percent composition of a compound, what is the empirical formula? 40%C, 6.7% H.53.3% . 3) Determine the limiting reactant (LR) and the...
Determine the mass (in g) of nitrogen gas that can be formed from 50.0 g dinitrogen tetraoxideand 45.0 g hydrazine (N2H4). What’s the reducing agent in the reaction? Show all work. No work, no credit. N2O4 (l) + 2 N2H4 (l) → 3 N2 (g) + 4 H2O (g)
Determine the limiting reactant and calculate the number of grams of nitrogen dioxide, NO, that can be formed when 105 g of nitrogen, N, reacts with 98.5 g of oxygen, N.(9) + 2 0,(9) - 2 NO (9)
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) +...
2,3,4,5
CHEM 1113: Recitation Activity - Week 3 Stoichiometry Learning Goals • Determine the limiting reactant and excess reactant for chemical reactions on the molecule scale. • Determine the amount of product that can be formed based on the starting amounts of a chemical system. • Calculate the amounts of reactants, products, or leftovers for chemical reaction problems with limiting and excess reactants in both moles and grams. Part I: Quantitative Aspects of Chemical Formulas 1. What is the mass...
How many grams of nitrogen gas are formed when 10.0 g of KNO3 decomposes according to the following reaction? The molar mass of KNO3 is 101.11 g/mol 4 KNO3(s) - 2 K2O(s) + 2 N2(8) + 5 O2(8) O 0.698 O 0.362 g 2.778 1.388