chemical engineering

Question

Anu Bhardwaj · Accepted Answer

Step 1:- The balanced equation is: C2H4 + 3O2 ⟶ 2CO2 + 2H2O Explanation:- To balance the chemical equation for the combustion of ethene (C2H4) with oxygen (O2) to form carbon dioxide (CO2) and water (H2O), we need to ensure that the number of atoms of each element is the same on both sides of the equation. Step 2:- b) Given: Moles of ethene (C2H4) = 250 moles Moles of oxygen (O2) = 3000 moles The balanced chemical equation for the combustion of ethene is: C2H4 + 3O2 ⟶ 2CO2 + 2H2O According to the balanced equation, 1 mole of ethene reacts with 3 moles of oxygen. For 250 moles of ethene, we would need 250 × 3 = 750 250 × 3 = 750 moles of oxygen. Explanation:- To determine the limiting reactant, we need to compare the moles of ethene and oxygen available and see which one runs out first. From the information given, we have 250 moles of ethene and 3000 moles of oxygen. Using the balanced equation, 1 mole of ethene reacts with 3 moles of oxygen. 250 × 3 = 750 250 × 3 = 750 moles of oxygen. Since we have more than enough oxygen (3000 moles), oxygen is in excess, and ethene is the limiting reactant. Step 3:- c) Given: Moles of ethene initially = 250 moles Moles of ethene at interruption = 60 moles The extent of the reaction can be calculated as the difference between the initial moles of ethene and the moles of ethene at the interruption. Extent of reaction = Initial moles of ethene - Moles of ethene at interruption Extent of reaction = 250 moles - 60 moles = 190 moles Explanation:- The extent of the reaction at interruption refers to how much of the reaction has occurred. Since ethene is the limiting reactant, all of it reacts. Thus, the extent of the reaction is the amount of ethene that has reacted, which is 250 − 60 = 190 250 − 60 = 190 moles. Step 3:- d) Given: Moles of ethene initially = 250 moles Moles of oxygen initially = 3000 moles Moles of ethene at interruption = 60 moles Since ethene is the limiting reactant, all of it will be consumed during the reaction. Therefore, we can use the stoichiometry of the balanced equation to determine the moles of products formed from ethene. From the balanced equation: 1 mole of ethene (C2H4) produces 2 moles of carbon dioxide (CO2) 1 mole of ethene (C2H4) produces 2 moles of water (H2O) So, at interruption: Moles of CO2 produced = Moles of ethene at interruption × (2 moles CO2 / 1 mole ethene) = 60  moles × 2  moles CO2 1  mole ethene = 120  moles CO2 = 60  moles × 1  mole ethene 2  moles CO2 ​ = 120  moles CO2 Moles of H2O produced = Moles of ethene at interruption × (2 moles H2O / 1 mole ethene) = 60  moles × 2  moles H2O 1  mole ethene = 120  moles H2O = 60  moles × 1  mole ethene 2  moles H2O ​ = 120  moles H2O Since oxygen is in excess, it doesn't limit the formation of products. Therefore, the moles of CO2 and H2O produced are only dependent on the moles of ethene reacted. Hence, at interruption: Moles of CO2 = 120 moles Moles of H2O = 120 moles For oxygen, since it's in excess, there will still be some remaining. The initial moles of oxygen were 3000 moles, and since only a portion of it reacted, we can find the remaining moles by subtracting the moles of oxygen used in the reaction: Moles of oxygen remaining = Initial moles of oxygen - Moles of oxygen used = 3000  moles − ( 250  moles ethene × 3  moles O2 1  mole ethene ) = 3000  moles − ( 250  moles ethene × 1  mole ethene 3  moles O2 ​ ) = 3000  moles − 750  moles = 2250  moles = 3000  moles − 750  moles = 2250  moles So, at interruption: Moles of O2 remaining = 2250 moles Therefore, at interruption: Moles of CO2 = 120 moles Moles of H2O = 120 moles Moles of O2 = 2250 moles Explanation:- To find out how many moles of each species are present at the interruption, we need to use the stoichiometry of the balanced equation. Since ethene is completely consumed, we only need to consider the products formed from it. From the balanced equation, for every 1 mole of ethene, we get 2 moles of CO2 and 2 moles of H2O. Final Answer:- a) Balanced equation: � 2 � 4 + 3 � 2 → 2 � � 2 + 2 � 2 � C 2 H 4 + 3 O 2 → 2 CO 2 + 2 H 2 O b) Limiting reactant: Ethene (C2H4) is the limiting reactant. c) Extent of reaction at interruption: 190 moles of ethene have reacted. d) Moles of each species present at interruption: Moles of CO2 = 120 moles Moles of H2O = 120 moles Moles of O2 = 2250 moles

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