1 mol NH3 1.00 mol O2 4.00 mol NO 1.50 mol H2O

1 mol NH3 1.00 mol O2 4.00 mol NO 1.50 mol H2O

1몰 암모니아와 1.00몰 산소가 반응하면 산화 질소와 물이 생성된다

 

 

One mol of ammonia reacts with 1.00 mol of oxygen

to form nitrogen oxide and water according to the reaction

4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)

State which statements are true about the reaction

and make the false statements true.

a) All the oxygen is consumed.

b) 4.00 mol NO are produced.

c) 1.50 mol H2O are produced.

d) The description of the experiment does not provide

enough information to determine percent yield.

e) Three moles of water are produced

for every two moles of NO obtained.

 

 

 

a) All the oxygen is consumed.

---> True

 

4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)

 

NH3 : O2 = 4 : 5 계수비(= 몰수비) 이므로,

1 mol NH3와 반응하는 O2의 몰수를 계산하면,

NH3 : O2 = 4 : 5 = 1 mol : ? mol

 

? = 5 / 4 = 1.25 mol O2

---> O2는 이만큼 없다, 부족하다?

---> O2 = 한계 반응물, NH3 = 과잉 반응물.

( 참고: 한계 반응물 https://ywpop.tistory.com/3318 )

 

 

 

b) 4.00 mol NO are produced.

---> False

 

한계 반응물이 생성물의 양을 결정하므로,

1.00 mol O2 반응 시,

생성되는 NO의 몰수를 계산하면,

O2 : NO = 5 : 4 = 1.00 mol : ? mol

 

? = 4 × 1.00 / 5 = 0.800 mol NO

 

 

 

c) 1.50 mol H2O are produced.

---> False

 

O2 : H2O = 5 : 6 = 1.00 mol : ? mol

 

? = 6 × 1.00 / 5 = 1.20 mol H2O

 

 

 

d) The description of the experiment does not provide

enough information to determine percent yield.

---> True

 

얻은 생성물의 양이 주어지지 않았다.

 

 

 

e) Three moles of water are produced

for every two moles of NO obtained.

---> True

 

NO : H2O = 4 : 6 = 2 mol : ? mol

 

? = 6 × 2 / 4 = 3 mol H2O

---> 2 mol NO 생성될 때(얻을 때), 3 mol H2O 생성.

 

 

 

 

[키워드] 한계 반응물 기준, 한계 시약 기준, 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l) 반응 기준, 4NH3 + 5O2 → 4NO + 6H2O 반응 기준