Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. termed hydrogenation, this type of reaction is used to produce products such as margarine. a typical hydrogenation reaction is c10h20() + h2(g) → c10h22(5) decene decane how much decane can be produced in a reaction of excess decene with 2.45 g hydrogen? give your answer in scientific notation. o *10 g decane

The mass of decane produced is

Explanation:

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

      ......(1)

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

The chemical equation for the hydrogenation of decene follows:

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

Hence, the mass of decane produced is

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.