For the reaction CH4 +2O2 = CO2 +H2O How many grams of water (H2O) are produced from the combustion of 6.35 moles of methane (CH4)? Please show all work.

reaction

CH₄  +  2 O₂  ==>  CO₂  + 2 H₂O   (Equal)

first, let's count the mole of H₂O that formed

mole H₂O = (coefficient of H₂O / coefficient of CH₄) x mole CH₄

mole H₂O = (2/1) x 6,35 mole

mole H₂O = 12,7 mole

so

Mass H₂O = mole H₂O x Molecular Mass

Mass H₂O = 12,7 mole x 18   ((2 x Ar H) + Ar O)

Mass H₂O = 228,6 g

  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 best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.