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

m=9

step-by-step explanation:

it is b that is the answer.