c2h2 + 2h2 → c2h6 suppose 20.0 mol of acetylene , 50.0 kmol of hydrogen and 50.0 kmol of ethene are charge into a batch of reactor . after some time 30.0 kmol of hydrogen has reacted . how much of each species will be present in the reactor at that moment?
To determine the amount of each species present in the reactor at that moment, we need to use stoichiometry and the concept of limiting reactant.
First, let's write down the balanced chemical equation for the given reaction:
C2H2 + 2H2 → C2H6
From the balanced equation, we can see that 1 mol of acetylene (C2H2) reacts with 2 mol of hydrogen (H2) to produce 1 mol of ethane (C2H6).
Given:
- 20.0 mol of acetylene (C2H2)
- 50.0 kmol of hydrogen (H2)
- 50.0 kmol of ethene (C2H4) [Note: ethene is not involved in the reaction, but it might be a typo]
After some time, 30.0 kmol of hydrogen (H2) has reacted. This means that 30.0 kmol of hydrogen has been consumed in the reaction.
Let's calculate the limiting reactant to determine the maximum amount of product formed. The limiting reactant is the reactant that is completely consumed first and limits the amount of product that can be formed. In this case, we are given the initial amounts of acetylene and hydrogen, so we need to compare their molar quantities.
Molar quantity of acetylene (C2H2): 20.0 mol
Molar quantity of hydrogen (H2): 50.0 kmol - 30.0 kmol = 20.0 kmol
Since the molar quantities of acetylene and hydrogen are equal (20.0 mol), both reactants are in stoichiometric balance. Therefore, neither reactant is limiting, and both will be completely consumed.
So, after the reaction, the amount of each species present in the reactor will be:
- 0 mol of acetylene (C2H2) since it is completely consumed
- 0 mol of hydrogen (H2) since it is completely consumed
- 50.0 kmol of ethene (C2H4), assuming it was not consumed or reacting with other substances