2HClO3 + Ni →Ni(ClO3)2 + H2 What volume at STP of Hydrogen gas will be produced from 12.34 grams of Nickel?

Volume of hydrogen produced = 4.485 L

Explanation:

Given data:

Volume of hydrogen produced = ?

Pressure = standard = 1 atm

Temperature = standard = 273.15 K

Mass of Ni = 12.34 g

Solution:

Chemical equation:

2HClO₃ + Ni     →     Ni(ClO₃)₂ + H₂

Number of moles of Ni:

Number of moles = mass / molar mass

Number of moles = 12.34 g / 58.69 g/mol

Number of moles = 0.2 mol

Now we will compare the moles of hydrogen with nickel.

                  Ni             :           H₂

                   1              :            1

                0.2            :           0.2

Volume of hydrogen:

PV = nRT

1 atm × V = 0.2 mol × 0.0821 atm.L/mol.K × 273.15 K

V = 4.485 atm.L/1 atm

V = 4.485 L

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

20 drops hope this