A mixture of hydrazine and hydrogen peroxide is used as a fuel for rocket engines. How many grams of hydrazine are needed to react with #0.453# moles of hydrogen peroxide?

The reaction is

#"N"_2"H"_4(l)+2"H"_2"O"_2(l) -> "N"_2(g)+4"H"_2"O"(g)#

Question

The reaction is

#"N"_2"H"_4(l)+2"H"_2"O"_2(l) -> "N"_2(g)+4"H"_2"O"(g)#

Wyatt Atkins · Accepted Answer

#"7.26 g N"_2"H"_4#

For starters, you know by looking at the balanced chemical equation

#"N"_ 2"H"_ (4(l)) + 2"H"_ 2"O"_ (2(l)) -> "N"_ (2(g)) + 4"H"_ 2"O"_ ((g))#

that every mole of hydrazine that takes part in the reaction consumes #2# moles of hydrogen peroxide. In other words, the two reactants take part in the reaction in a #1:2# mole ratio.

You already know that the reaction consumed #0.453# moles of hydrogen peroxide, so use this mole ratio to figure out how many moles of hydrazine reacted

#0.453 color(red)(cancel(color(black)("moles H"_2"O"_2))) * ("1 mole N"_2"H"_4)/(2color(red)(cancel(color(black)("moles H"_2"O"_2)))) = "0.2265 moles N"_2"H"_4#

To convert this to grams, use the molar mass of hydrazine

#0.2265 color(red)(cancel(color(black)("moles N"_2"H"_4))) * "32.045 g"/(1color(red)(cancel(color(black)("mole N"_2"H"_4)))) = color(darkgreen)(ul(color(black)("7.26 g")))#

The answer is rounded to three sig figs, the number of sig figs you have for the number of moles of hydrogen peroxide.

Wyatt Adkins · Answer

undefined To determine the number of grams of hydrazine needed to react with 0.453 moles of hydrogen peroxide, you need to use the balanced chemical equation for the reaction between hydrazine (N2H4) and hydrogen peroxide (H2O2). The balanced equation is:

N2H4 + H2O2 -> N2 + 2H2O

From the balanced equation, it can be seen that one mole of hydrazine reacts with one mole of hydrogen peroxide. Therefore, the number of moles of hydrazine needed will be equal to the number of moles of hydrogen peroxide, which is 0.453 moles.

Now, you can use the molar mass of hydrazine (N2H4), which is approximately 32.05 g/mol, to convert moles to grams:

0.453 moles of N2H4 × (32.05 g/mol) = 14.51 grams of N2H4

Therefore, approximately 14.51 grams of hydrazine are needed to react with 0.453 moles of hydrogen peroxide.

A mixture of hydrazine and hydrogen peroxide is used as a fuel for rocket engines. How many grams of hydrazine are needed to react with #0.453# moles of hydrogen peroxide?

The reaction is #"N"_2"H"_4(l)+2"H"_2"O"_2(l) -> "N"_2(g)+4"H"_2"O"(g)#

The reaction is

#"N"_2"H"_4(l)+2"H"_2"O"_2(l) -> "N"_2(g)+4"H"_2"O"(g)#