Calculate the mass in grams of CO2 are formed if 89.6 liters of CH4 are used up at S. T.P?
(Hint: At S. T.P., one mole of any gas occupies a
volume of 22.4 liters).

Mass = 176 g

Explanation:

Given data:

Volume of CH₄ = 89.6 L

Mass of CO₂ formed = ?

Solution:

Chemical equation:

CH₄ + 2O₂    →       CO₂ + 2H₂O

one mole of any gas at STP occupy 22.4 L volume.

number of moles of CH₄  that occupy 89.6 L = 89.6/22.4 = 4 mol

Now we will compare the moles of CH₄ and CO₂:

                CH₄            :          CO₂

                  1               :            1

                  4              :             4

Mass of CO₂:

Mass = number of moles × molar mass

Mass = 4 mol × 44 g/mol

Mass = 176 g

the increase of protons   hope this

a gas, having a molecular weight of 13 kg/kmol and a kinematic viscosity of 0.25 cm2/s, flows through a pipe 0.25 m internal diameter and 5 km long at the rate of 0.4 m3/s and is delivered at atmospheric pressure.