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Chapter 4: 4.1 CYL (page 177)

Write a balanced equation for the decomposition of ammonium nitrate to form molecular nitrogen, molecular oxygen and water. (Hint Balance oxygen last, since it is present in more than one molecule on the right side of the equation)

Short Answer

Expert verified

The balanced equation will be \(2N{H_4}N{O_3} \to 2{N_2} + {O_2} + 4{H_2}O.\)

Step by step solution

01

Writing unbalanced equation with unknown constants

\(wN{H_4}N{O_3} \to x{N_2} + y{O_2} + z{H_2}O,\) where w, x, y, and z, are unknown constants.

02

Determine the balanced equation

Count the number of times each element appears on either side of the reaction.

Reactants N= 2w, H= 4w, O= 3w.

Products N=2x, O= 2y+z, H= 2z.

2w = 2x鈥︹�︹�︹�︹�︹�︹�︹�︹��..(i)

4w = 2z鈥︹�︹��..鈥︹�︹�︹�︹�︹��.(ii)

3w = 2y+z鈥︹�︹�︹��...鈥︹�︹�︹��.(iii)

Now, from equation (i):

w = x

From equation (ii):

2w = z

And putting value of 鈥渮鈥� in (iii), we get:

3w = 2y + 2w

w = 2y

Let y=1 then,

w = 2 x 1

= 2.

x = 2

z = 2 x 2

= 4.

Therefore, the balanced equation is \(2N{H_4}N{O_3} \to 2{N_2} + {O_2} + 4{H_2}O.\)

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Write a balanced molecular equation describing each of the following chemical reactions.

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