complete the first, second, third, fourth, fifth and six rows. 2 Secure I https/
ID: 252600 • Letter: C
Question
complete the first, second, third, fourth, fifth and six rows. 2 Secure I https//session.masteringchemistry.com/myct/item Chapter 7 Exercise 7.40 Constants | Periodic Table Consider the following balanced equation 2 N2H4 (9) N20,(9) 32(9) 4 H20(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 product that is made. Mol N2Hs Mol N204 Mol N2 Mol H20 9 3.5 4.5 12.7Explanation / Answer
We solve this by using ratios. From the equation
2 N2H4 +1 N2O4-------> 3 N2 + 4 H2O
we can see that for 1 mole (2/2 moles) N2H4, 1/2 moles of N2O4 are used and 3/2 or 1.5 moles of N2 and 4/2 or 2 moles of H2O are produced. SO if you have 4 moles of N2H4, 4 x 1/2 or 2 moles of N2O4 will be used and 4 x 1.5= 6 moles of N2 and 4 x 2= 8 moles of H2O are produced.
Similarly if 1 mole (4/4 moles) of water is produced, then there will be 2/4(or 1/2) moles of N2H4, 1/4 moles of N2O4 and 3/4 moles of N2. So if 18 moles of water are produced then 18 x 1/2= 9 moles of N2H4, 18 x 1/4= 4.5 moles of N2 O4 and 18 x 3/4= 13.5 moles of N2 will be used.
The same procedure is used to calculate all the rest.
Mol N2H4 Mol N2O4 Mol N2 Mol H2O 4 2 6 8 18 9 27 36 9 4.5 13.5 18 3.5 1.75 5.25 7 9 4.5 13.5 18 8.47 4.23 12.7 16.93Related Questions
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