How many grams of H2 gas are produced if 48
grams of CH4 gas are consumed?

Mass = 12.12 g

Explanation:

Given data:

Mass of CH₄ = 48 g

Mass of H₂ produced = ?

Solution:

Chemical equation:

CH₄ →   C + 2H₂

Number of moles of CH₄:

Number of moles = mass/molar mass

Number of moles = 48 g/ 16 g/mol

Number of moles = 3 mol

Now we will compare the moles of CH₄  and H₂.

               CH₄          :           H₂

                  1             :           2

                  3            :          2/1×3 = 6 mol

Mass of  H₂:

Mass = number of moles × molar mass

Mass = 6 mol × 2.02 g/mol

Mass = 12.12 g

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :

58750.08068 is the answer i think