Consider the reaction ch4 + o2 co2 + h2o balance the equation the number of grams of water formed when 32 grams of methane ch4 is burned

72 g  

Step-by-step explanation:

a) Balanced equation

We know we will need an equation with masses and molar masses, so let’s gather all the information in one place.  

M_r:  16.04                           18.02

          CH₄ + 2O₂ ⟶ CO₂ + 2H₂O  

m/g:    32

(b) Mass of H₂O

(i) Calculate the moles of CH₄

n = 32 g CH₄  × (1 mol CH₄/16.04 CH₄)

  = 2.00 mol CH₄

(ii) Calculate the moles of H₂O

The molar ratio is (2 mol H₂O /1 mol CH₄)

n = 2.00 mol CH₄ × (2 mol H₂O /1 mol CH₄)

  = 3.99 mol H₂O

(iii) Calculate the mass of H₂O

m = 3.99 mol H₂O × (18.02 g H₂O /1 mol H₂O)

m = 72 g H₂O

The reaction produces 72 g H₂O.

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-

the answer would be b i believe