Question

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)

Answer 1

Here is what I solved before, please modify the figures as per your question. Please let me know if you have further questions. Ifthis helps then kindly rate 5-stars.

Given the following chemical equation, determine how many grams of N2 are produced by 8.04 g of H2O2 and 5.23 g of N2H4.

2H202 (l)+ N2H4 (l) -----> 4H20 (g) + N2 (g)

2H202 (l)+ N2H4 (l) -----> 4H20 (g) + N2 (g)

molar mass of 1) H2O2 = 34 g/mole

2) N2H4 = 32 g/mole

3) H2O = 18 g/mole

4) N2 = 28 g/mole

now, moles of H2O2 in 8.04 g of it = 8.04/34 = 0.2365 moles

  moles of N2H4 in 5.23 g of it = 5.23/32 = 0.1634 moles

now, as per the balanced reaction equation 2 moles of H2O2 requires 1 mole of N2H4

therefore, 0.2365 moles of H2O2 requires 0.11825 mols of N2H4

clearly N2H4 is in excess and H2O2 is the limiting reagent

thus the product will depend on the moles of H2O2

now, 2 moles of H2O2 forms 1 mole of N2

therefore, 0.2365 moles of H2O2 forms 0.2365/2 = 0.11825 moles of N2

thus mass of N2 = moles of N2 formed * molar mass of N2 = 3.311 g