Question

For the balanced reaction: N2(g) + 3H2(g) → 2NH3(g). How many moles of NH, will be produced when 0.50 mol N2 reacts with 1.0 mol H,? A. 0.67 mol 2.0 mol 14. Calculate the mass of Co, formed when 2.3 g of ethanol, C2H^OH reacts with 3.2 g oxygen O, to form CO2, and H2O. (You balanced the reaction in 8.e)! This is a limiting reagent problem! A. 4.6g 6.6g B. 1.0 mol C. 0.50 mol E. 3.0 mol B. 2.2g C. 4.4g E. 2.93g

Answer 1

Answer:

First question: 0,67 moles

Second question: 4.4g

Explanation:

N2(g) + 3H2(g) → 2NH3(g)

For every mole of nitrogen, 3 moles of hydrogen reacts so I have 0,5moles.

By the rule of three:

1 N2 _______ 3H2

0,5 N2 _____ (0,5 m . 3m ) /1 m = 1,5 moles H2

For 3 moles of hydrogen, 1 mole of nitrogen reacts, so I have 1 mol

3 H2 _____ 1 N2

1 H2 _____ (1 m . 1 m) / 3m = 0,3 moles N2

I have 1 mole of H2 and I should use 1,5 moles and I have 0,5 moles of N2 but i should use 0,3 moles, so my limiting reagent is the H2

3H2 reacts to form 2NH3

1 H2 reacts to form x ---> (1 m . 2m) / 3m = 0,66666

C2H^OH + 2O2 ---> 2CO2 + H2O (that's the ballanced reaction)

Molar mass C2H^OH = 42,03 g/m

Molar mass O2 = 32 g/m

Moles C2H^OH = 2, 3 g / 42,03 g/m = 0,0547 m

Moles O2 = 3,2g / 32 g/m = 0,1 m

For 1 mol ethanol reacts 2O2

0,0547 mol reacts ____ = (0,0547 m . 2 m) / 1m = 0,1094 m

O2 is my limiting reagent because I have to use 0,1094 m and I only have 0,1 m.

So in the reaction 2 mol O2 __ makes __ 2 moles CO2                    

                            0,1 moles ___ makes __ = 0,1 moles

The ratio is 1 to 1

Molar mass CO2 = 44g/m so mass CO2 formed is moles x molar mass

44g/m . 0,1 m = 4,4g