There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC2(s) + 2 H2O(g) → C„H,(9) + Ca(OH)2(s) AH=-414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H2(9) + 3 CO2(9) + 4 H2O(9) → 5 CH,CHCO,H(9) AH=132. kJ Calculate the net change in enthalpy for the formation of one mole of acrylic acid from calcium carbide, water and carbon dioxide from these reactions. Round your answer to the nearest kJ.

There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC2(s) + 2 H2O(g) → C„H,(9) + Ca(OH)2(s) AH=-414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H2(9) + 3 CO2(9) + 4 H2O(9) → 5 CH,CHCO,H(9) AH=132. kJ Calculate the net change in enthalpy for the formation of one mole of acrylic acid from calcium carbide, water and carbon dioxide from these reactions. Round your answer to the nearest kJ.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

48.2 mL of a solution of HCl is combined with 110.7 mL of 1.35 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C, and the final temperature after reaction is 29.3°C. What is the molarity of the HCl solution? You may assume that there is an excess of base (so that all the HCI has reacted), that the specific heat of the reaction mixture is 0.96 cal/g °C, and that the density of the reaction mixture is 1.02 g/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mole.
The reaction between HCl and NaOH is represented below. When equal volumes of 1.00 M NaOH and 1.00 M HCl are mixed, 57.1 kJ of heat is released. What would A H be if 2.00 M HCI and 2.00 M NaOH is used instead of 1.00 M? HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l) AH = -57.1 kJ/mol... (A) - 28.6 kJ B-85.7 kJ (c) -57.1 kJ D - 114 kJ
In the following reaction, how much heat is generated when 3.21 moles of CH4 are burned? CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g) AH° = -802 kJ/mol
How much heat is released when an excess of Fe reacts with 48 g of 02 (M = 32 g/mol), according to the following reaction: 4Fe(s) + 302(8) → 2Fe,O3(s) AH = -1652 kJ 826 kJ O 1041 kJ O 2478 kJ O 1652 KJ
Iron can be extracted from the iron(III) oxide found in iron ores (such as haematite) via an oxidation-reduction reaction with carbon. The thermochemical equation for this process is: 2 Fe203(s) + 3 C(s) → 4 Fe(1) + 3 CO2(g) AH° = +467.9 kJ
In a coffee-cup calorimeter, 59.0 mL of 0.100 M AgNO3 and 59.0 mL of 0.100 M HCI are mixed to yield the following reaction. Ag (aq) + Cl(aq) → AgCl(s) The two solutions were initially at 19.10°C, and the final temperature is 19.90°C. Calculate the heat that accompanies this reaction in kJ/mol of AgCl formed. Assume that the combined solution has a mass of 118.0 g and has a specific heat capacity of 4.18 1/°C 9- 407 kJ/mol
4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).
Consider the following reaction: 2Mg(s)+O2(g)⟶2MgO(s)ΔH∘=−1203kJ What mass of magnesium must be combusted in order to generate 174.0 kJ of heat?
Calculate AH for the reaction P4010(s) + 6PC15(g) – 10C13PO(g) given, P4(s) + 6C12(g) → 4PC13(g) AH = -1225.6 kJ P4(s) + 502(g) – P4010(s) AH = -2967.3 kJ PC13(g) + Cl2(g) → PC15(g) AH = -84.2 kJ PC13(g) + (1/2)02(g) – C13PO(g) AH=-285.7 kJ ΔΗ- kJ
Consider the following chemical reaction: What is AH for the following reaction? 2Mg(s) + O₂(g) → 2MgO(s); AH = -1204KJ 4MgO 4Mg(s) + 20₂(g); AH =
*ONLY THE SECOND PART*
In the following reaction, how many grams of CH3OH are required to produce 1.578 x 10° kJ of heat? 2 CH3OH (1) +3 O2 (g) → 2 CO2 (g) + 4 H2O(g) AH = -1280. kJ/mol Please do not include units in your answer.