50.0 g N2O4 reacts with 45.0 g N2H4. Determine the percent yield if 12.5 g of N2 are actually formed.
N2O4(l) + 2N2H4(l) ---> 3N2(g) + 4H2O(g)
50.0 g N2O4 reacts with 45.0 g N2H4. Determine the percent yield if 12.5 g of...
How many grams of which reactant will remain unreacted when 10.0 g of N2H4(l) reacts with 15.0 g of N2O4(l) in the following reaction? 2N2H4(l) + N2O4(l) → 3N2(g) + 4H2O(g) Assume 100% yield. 4.78 g of N2H4 2.39 g of N2H4 0.01 g of N2O4 0.64 g of N2O4 0.22 g of N2H4 Step by Step, Thanks!
Consider the reaction between N2H4 and N2O4: 2N2H4(g)+N2O4(g)?3N2(g)+4H2O(g) A reaction vessel initially contains 21.0 g N2H4 and 74.9 g of N2O4. Hint: The limiting reactant is completely consumed, but the reactant in excess is not. Use the amount of limiting reactant to determine the amount of products that form and the amount of the reactant in excess that remains after complete reaction. Part B: Calculate the mass of N2O4 that will be in the reaction vessel once the reactants have...
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
For the reaction 2N2H4 (l) + N2O4 (l) → 3N2 (g) + 4H2O(l), determine the mass of H2O formed when 20.0 grams of N2O4 react. A) 3.6 grams B) 7.8 grams C) 8.6 grams D) 15.6 grams
Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other...
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)
Consider the balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the other reactant, as well as the moles of each product formed. If the number of moles of a product is provided, fill in the required amount of each reactant to make that amount of product, as well as the amount of the other product that...
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...
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...