Question

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 is made.

mol N2H4	mol N2O4	mol N2	mol H2O
2	_____	_____	_____
_____	6	_____	_____
_____	_____	_____	10
2.5	_____	_____	_____
_____	4.2	_____	____
_____	_____	14.5	_____

Answer 1

The given reaction is 2N,H, (g)+N,O4(g) +3N2(g) + 4H2O(g) Here, comparing the stoichiometry as follows: 1. since, mol of N H = 2, the reaction will be same. 2. Since, given N,H,= 6, that is triple of the reaction so everything will be triple. 3. Since, mol of H,O=10, that is 10/4 = 2.5times, so everything will be multiplied by 2.5. 4. Since, mol of N,O,= 2.5 which is 2.5/2= 1.25, so everything will be multiplied by 1.25. 5. Since, mol of N,O,= 4.2 which is 4.2/1=4.2, so everything will be multiplied by 4.2. 6. Since, mol of N, = 14.5 which is 14.5/3 =4.83, so everything will be multiplied by 4.83. Hence, the table is as follows: moles N, H N ,0 N2 HO 126 24 2.5 10 | 1.25 | 18 7.5 3.74 12.6 14.5 2.5 8.4 9.66 5 4.2 4.83 16.8 19.32