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

each  column  of the  table  is called a group. elements in a group share similar properties. groups are  read  from  top  to  bottom. metal. metalloid. nonmetal. solid. liquid. gas. fe. hg. o.  2. 3. 4. 5. 6. 7. 8. 9.  2. beryllium. 9.012. 4.  sodium. 22.990.  11. 3.  magnesium. 24.305.  12.  potassium. 39.098.  19. 4.  calcium. 40.078.  20. i guess  i