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

the dependant variable is spilled water

the independent is the heat

58750.08068 is the answer i think