Answer:
0.4209 g
Step-by-step explanation:
Given Data:
Balanced given reaction is
2NO(g) + O2(g) → 2NO2(g)
Grams of oxygen (O2 ) = to find that produce 1.21 g of NO2
Solution:
Data showed by a balance equation
2NO(g) + O2(g) ----------------------→ 2NO2(g)
1 mole 1 mole 2 mole
From the reaction it is clear that 1mole of oxygen give 2mole of NO2
From formula we can calculate weight in grams for oxygen as well as for NO2
Mole= weight in grams/molecular weight (mass)………..(1)
Calculation for the weight in gram for oxygen
Mole= weight in grams of O2 /molecular weight (mass) of O2…………. (2)
Put values in formula 2
1 Mole of oxygen = weight in grams of O2 / 16x2
1 Mole oxygen = weight in grams of O2 / 32
= Weight in grams of O2 = 32grams
Calculation for the weight in gram for NO2
Mole= weight in grams of NO2 /molecular weight (mass) of NO2…………. (2)
Put values in formula 2
2 Mole NO2 = weight in grams of NO2 / 14+ (16x2)
2 Mole NO2 = weight in grams of NO2 / 46
= Weight in grams of NO2 = 46x2
= Weight in grams of NO2 = 92grams
Now coming back to balance Reaction by representing moles in grams
2NO(g) + O2(g) ----------------------→ 2NO2(g)
1 mole 1 mole 2 mole
32g 92g
By applying unity formula
If 32g of O2 gives ………………….92g of NO2
So how many grams of oxygen will produce 1.21g of NO2
X gram of O2 = 32x 1.21/92
= X gram of O2 = 32x 1.21/92
= X gram of O2 = 0.4209 g
So 0.4209 g required to produce 1.21g of NO2