mass A moles A moles B particles B Referring to the equation above, how many grams of CH3OH must react in order to produce 17.5 g of H2O

17.5 g H2O x 1 mol H2O / 18.01 g H2O x 2 mol CH3OH / 4 mol H2O x 32.04 g CH3OH / 1 mol CH3OH = 15.5 g CH3OH

Explanation:

Hi Bash!

I believe we're in the same class because I was trying to understand this as well.

You have a missing piece of information which is the chemical equation the question is derived from. At the top of the study guide, you will find that the equation is: 2 CH3OH    +    3 O2      -->       2 CO2   +  4 H2O

The given is 17.5 g of H2O and you're trying to find how many grams of CH3OH must react.

You'll begin by converting the grams of H2O into moles: 17.5 g H2O x 1 mol H2O/18.01 g H2O (18.01 is the molar mass and each mole has a mass of 18.01 g)

Then you will convert the moles of H2O into moles of CH3OH. There are 2 moles of CH3OH as seen in the reactant and there are 4 moles of H2O as seen in the product side : 2 mol CH3OH / 4 mol H2O x 32.04 g CH3OH / 1 mol CH3OH.

Combine all these steps together and you will get: 17.5 g H2O x 1 mol H2O / 18.01 g H2O x 2 mol CH3OH / 4 mol H2O x 32.04 g CH3OH / 1 mol CH3OH = 15.5 g CH3OH

radioactive decay occurs in unstable atomic nuclei – that is, ones that don't have enough binding energy to hold

the nucleus together due to an excess of either protons or neutrons.

d.) the average kinetic energy of the gas particles is greater in container b because its particles move faster.