How many grams of methanol are produced when 14 grams of carbon monoxide reacts with 1.5 grams of hydrogen gas?

The mass of methanol produced is 12 grams

Explanation:

To calculate the number of moles, we use the equation:

    .....(1)

Given mass of carbon monoxide = 14 g

Molar mass of carbon monoxide= 28 g/mol

Putting values in equation 1, we get:

Given mass of hydrogen gas = 1.5 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1, we get:

The chemical equation for the reaction of carbon monoxide and hydrogen gas follows:

By Stoichiometry of the reaction:

2 moles of hydrogen gas reacts with 1 mole of carbon monoxide

So, 0.75 moles of hydrogen gas will react with = of carbon monoxide

As, given amount of carbon monoxide is more than the required amount. So, it is considered as an excess reagent.

Thus, hydrogen gas is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of hydrogen gas produces 1 mole of methanol

So, 0.75 moles of hydrogen gas will produce = of methanol

Now, calculating the mass of methanol from equation 1, we get:

Molar mass of methanol = 32 g/mol

Moles of methanol = 0.375 moles

Putting values in equation 1, we get:

Hence, the mass of methanol produced is 12 grams

a). in this case, dh> 0 and sd> 0. if t becomes larger, the term "-tds" will become more negative. at some point, it is possible that -dts will be more negative than the dh is positive, and the reaction will become spontaneous. this is probably the correct answer, but you should look at all of the other possibilities and make sure of that.