Question

In: Chemistry

A) According to the (unbalanced) reaction: NH3(g) + O2(g) ----> NO2 (g) + H20 (l) What...

A) According to the (unbalanced) reaction: NH3(g) + O2(g) ----> NO2 (g) + H20 (l)

What volume of NO2(g) will be produced from the combustion of 521 g of O2(g), assuming the reaction takes place at standard temperature and pressure?

B) What mass of water will be produced if a 38.1 L sample of ammonia at 1.13 atm of pressure and. 23.1 degree celcius reacts completely?

Expert Solution

A)

Molar mass of O2 = 32 g/mol

mass of O2 = 5.21*10^2 g

mol of O2 = (mass)/(molar mass)

= 5.21*10^2/32

= 16.28 mol

Balanced chemical equation is:

4NH3 + 7O2 = 4NO2 + 6H2O

According to balanced equation

mol of NO2 formed = (4/7)* moles of O2

= (4/7)*16.28

= 9.304 mol

At STP, molar volume is 22.4 L/mol

Now use:

volume = number of mol * molar volume

= 9.304 mol * 22.4 L/mol

= 208 L

Answer: 208 L

B)

Given:

P = 1.13 atm

V = 38.1 L

T = 23.1 oC

= (23.1+273) K

= 296.1 K

find number of moles using:

P * V = n*R*T

1.13 atm * 38.1 L = n * 0.08206 atm.L/mol.K * 296.1 K

n = 1.772 mol

From equation,

mol of H2O = (6/4)*number of mol of NH3 reacted

= (6/4)* 1.772

= 2.658 mol

Molar mass of H2O,

MM = 2*MM(H) + 1*MM(O)

= 2*1.008 + 1*16.0

= 18.016 g/mol

use:

mass of H2O,

m = number of mol * molar mass

= 2.658 mol * 18.02 g/mol

= 47.89 g

Answer: 47.9 g

queen_honey_blossom answered 1 year ago

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