Question

For the reaction represented by the equation 2h+O2– 2H2O, how may grams of water are produced from 6.00 mol of hydrogen?

Atomic mass of hyorogen = 1.0gmol
Atomic mass of oxygen = 16.0 omo

Answer 1

To produce 6.00 mol of hydrogen, 3.00 mol of oxygen is required.

Step-by-step explanation:

Solution:

First, we need to look at the reaction involved. Hydrogen and oxygen react to form water. Two moles of hydrogen react with one mole of oxygen to give two moles of water.

From the balanced chemical equation, we can see that 1 equivalent of oxygen produces 2 equivalents of water. We can therefore write the following ratio: 1 mol O₂ : 2 mol H₂O. To find the amount of oxygen needed to produce 6.00 mol of hydrogen, we can set up the following proportion:

1 mol O₂ / 2 mol H₂O = x mol O₂ / 6.00 mol H₂

Solving for x, we find that x = 3.00 mol O₂.

Answer 2

Mass = 108 g

Step-by-step explanation:

Given data:

Mass of water produced = ?

Number of moles of hydrogen = 6.00 mol

Solution:

Chemical equation:

2H₂ + O₂ → 2H₂O

Now we will compare the moles of hydrogen with water.

H₂ : H₂O

2 : 2

6 : 6

Mass of water:

Mass = number of moles × molar mass

Mass = 6 mol × 18 g/mol

Mass = 108 g