Question

for the chemical reaction

2H_{2}O_{2} (l)
+N_{2}H_{4}(l)--->4H_{2}O(g)+N_{2}(g)

determine how many grams of N2 are produced from the reaction of
8.62 g of H2O2 and 6.95 g of N2H4.

Answer #1

Mass of H_{2}O_{2} = 8.62 g

Molar mass of H_{2}O_{2} = 34.0147 g/mol

Moles of H_{2}O_{2} = mass/ Molar mass = 8.62
g/(34.0147 g/mol) = 0.253 mol

Mass of N_{2}H_{4} = 6.95 g

Molar mass of N_{2}H_{4} = 32.0452 g/mol

Moles of N_{2}H_{4} = 6.95g/ (32.0452 g/mol) =
0.217 mol

From reaction,

2 mol of H_{2}O_{2} reacts with 1 mol of
N_{2}H_{4}

Thus, 0.253 mol of H_{2}O_{2} reacts with
0.253*1/2 = 0.127 mol of N_{2}H_{4}

So, H_{2}O_{2} is a limiting reagent.

2 mol of H_{2}O_{2} produces 1 mol of
N_{2}

Thus, moles of N_{2} produced from 0.253 mol of
H_{2}O_{2} = 0.127 mol

Molar mass of N_{2} = 28.0134 g/mol

Mass of N_{2} produced = moles* molar mass = 0.127
mol*28.0134 g/mol = **3.55g**

For the chemical reaction
2H2O2(l)+N2H4(l)------->4H2O(g)+N2(g)
Determine how many grams of N2 are produced from the reaction of
9.27 g of H2O2 and 5.99 g of N2H4.

Given the following chemical equation, determine how many grams
of N2 are produced by 9.75 g of H2O2 and 6.99 g of N2H4?
2H2O2(l)+N2H4(l)=4H2O(g)+N2(g)

determine how many grams of N2 are produced from the reaction of
9.39 g of H2O2 and 6.50 g of N2H4.

determine how many grams of N2 are produced from the reaction of
9.70 g of H2O2 and 5.08 g of N2H4.

How many moles of N2 can form when 0.412 mol of N2H4(l) reacts
with 0.195 mol of N2O4(l) in the following reaction 2N2H4(l) +
N2O4(l) → 3N2(g) + 4H2O(g) when the yield is 78.2%?

How many grams of hydrazine, N2H4, can be made from 10.39 g of
N2 and excess H2?

1. Consider the following chemical reaction:
2CH3OH(l) + 3O2 (g) → 2CO2 (g) + 4H2O(l)
Calculate the number of moles of CO2 produced when 11.25 mL of
methanol CH3OH reacted completely with O2 (g). The density of
methanol is 0.79 g/mL.

Consider the reaction between N2H4 and N2O4:
2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) A reaction vessel initially
contains 20.5 gN2H4 and 74.9 g of N2O4.
Calculate the mass of N2H4
Calculate the mass of N2O2
Calculate the mass of N2
Calculate the mass of H2O
that will be in the reaction vessel once the reactants have
reacted as much as possible. (Assume 100% yeild).

If 2.85 g of N2H4 reacts and produces 0.850 L of N2, at 295 K
and 1.00 atm, what is the percent yield of the reaction?
N2H4 (aq) + O2 (g) --> N2 (g) + 2H20 (l)

Determine how many grams of CO2 are produced by burning 7.49 g
of C4H10. _____g carbon dioxide and Balance the chemical equation
for this combustion reaction.

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