CH4 + 202 + CO2 + 2H2O
How many grams of CO2 will be produced from 15.0 g of CH4 and 114 g of O2?

Mass =41.36 g

Explanation:

Given data:

Mass of CH₄ = 15 g

Mass of O₂ = 114 g

Mass of CO₂ produced = ?

Solution:

Chemical equation:

CH₄ + 2O₂    →  CO₂ + 2H₂O

Number of moles of CH₄:

Number of moles = mass/ molar mass

Number of moles = 15 g /16 g/mol

Number of moles = 0.94 mol

Number of moles of O₂:

Number of moles = mass/ molar mass

Number of moles = 114 g /32 g/mol

Number of moles = 3.6 mol

Now we will compare the moles of CO₂ with both reactant.

                            O₂             :            CO₂

                             2              :               1

                             3.6           :          1/2×3.6= 1.8 mol

                         CH₄              :            CO₂

                            1                :               1

                         0.94            :           0.94

Number of moles of CO₂ produced by CH₄ are less so it will limiting reactant.

Mass of CO₂:

Mass = number of moles × molar mass

Mass = 0.94 mol × 44 g/mol

Mass =41.36 g

alkaline metals are lithium, sodium, rubidium, potassium, cesium and francium.

alkali metals have electronegativity from 0.7 to 1, lowest in periodic table of elements, which means that alkali metals (i group in periodic table) has positive oxidation number in compounds.

electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons towards itself.

alkaline metals (far left in main group) have lowest ionizations energy and easy remove valence electrons,

for example, potassium is the alkali metal and has a single valence electron in the outer electron shell.

electron configuration of potassium is: ₁₉k 1s²2s²2p⁶3s²3p⁶4s¹.

they can not exist alone in nature, because they are very reactive.

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