Balance this equation. If a coefficient of "1" is required, choose "blank" for that box. CH 4 + ___ O 2 → CO 2 + H 2 O

CH4 + 2O2 → CO2 + 2H2O

Explanation:

CH4 + O2 → CO2 + H2O

Left Side

C = 1

H = 4

O = 2

Right Side

C = 1

H = 2

O = 3

Ok so we'll balance the H first

CH4 + O2 → CO2 + 2H2O

Left Side

C = 1

H = 4

O = 2

Right Side

C = 1

H = 4

O = 4

Now we'll balance the O

CH4 + 2O2 → CO2 + 2H2O

Left Side

C = 1

H = 4

O = 4

Right Side

C = 1

H = 4

O = 4

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.