4.14 The combustion of liquid chloroethylene, C 2 H 3 Cl, yields carbon dioxide, steam, and hydrogen chloride gas. (a) Write a balanced equation for the reaction. (b) How many moles of oxygen are required to react with 35.00 g of chloroethylene? (c) If 125.00 g of chloroethylene reacts with an excess of oxygen, how many grams of each product are formed?
4.14 The combustion of liquid chloroethylene, C2H3Cl, yields carbon dioxide, steam, and hydrogen chloride gas. (a) Write a balanced equation for the reaction. (b) How many moles of oxygen are required to react with 35.00 g of chloroethylene? (c) If 125.00 g of chloroethylene reacts with an excess of oxygen, how many grams of each product are formed?
a.
Expert Solution
Interpretation Introduction
To determine:
The balanced chemical equation.
Explanation of Solution
In the combustion the chloroethylene, C2H3Cl reacts with oxygen. The combustion of C2H3Cl
produces carbon dioxide, steam, and hydrogen chloride gas, so that, the balanced equation is:
C2H3Cl(l) + 52O2(g)→2CO2(g)+H2O(g)+HCl(g)
b.
Expert Solution
Interpretation Introduction
To determine:
Moles of oxygen required to react with 35.00 g of chloroethylene.
Calculate the grams of CO2, H2O,andHCl that react with 1 mol of C2H3Cl in the reaction
2 mol CO2×44 g CO21 mol CO2=88 g CO21 mol H2O ×18 g H2O1 mol H2O=18 g H2O1 mol HCl ×36.5 g HCl1 mol HCl=36.5 g HCl
Calculate the grams of CO2, H2O,andHCl that are produced with 25.00 g of C2H3Cl.
62.5 g C2H3Cl-----------88 g CO225.00 g C2H3Cl----------- 25.00 g C2H3Cl × 88 g CO262.5 g C2H3Cl= 35.2 g CO262.5 g C2H3Cl-----------18 g H2O25.00 g C2H3Cl----------- 25.00 g C2H3Cl × 18 g H2O62.5 g C2H3Cl= 7.2 g H2O62.5 g C2H3Cl-----------36.5 g HCl25.00 g C2H3Cl----------- 25.00 g C2H3Cl × 36.5 g HCl62.5 g C2H3Cl= 14.6 g HCl
Conclusion
According to the following reaction,
a. C2H3Cl(l) + 52O2(g)→2CO2(g)+H2O(g)+HCl(g)
b. 35.00 g of C2H3Cl reacts with 1.4 moles of O2.
c. 25.00 g produces 35.2 g of CO2, 7.2 g of H2O and 14.6 g ofO2.
Want to see more full solutions like this?
Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!
If 5.9 × 10²⁵ molecules of CO₂ are produced in a combustion reaction, what is the mass in kg of CO₂ that is produced?
Propane (C3H8) is a component of natural gas and is used in domestic cooking and heating.
(a) Balance the following equation representing the combustion of propane in air: C3H8 + O2 ==> CO2 + H2O(b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reagent in this reaction.
The combustion of glucose is represented by the following balanced equation: C6H12O6 + 6 O2 --> 6 H2O + 6 CO2.
which reactant is the limiting reagent if there is 1 gram of both C6H12O6 and O2?
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY