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: CaC,(s) + 2 H,0(g) → C,H,(9) + Ca(OH),(s) AH=-414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H,(9) + 3 CO,(9) + 4 H,O(g) 5 CH,CHCO,H(9) AH=132. kJ Calculate the net change in enthalpy for the formation of one mole of acry!ic 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: CaC,(s) + 2 H,0(g) → C,H,(9) + Ca(OH),(s) AH=-414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H,(9) + 3 CO,(9) + 4 H,O(g) 5 CH,CHCO,H(9) AH=132. kJ Calculate the net change in enthalpy for the formation of one mole of acry!ic 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

Calcium carbonate, CaCO3 is used as a calcium supplement. When it is heated, it decomposes to form calcium oxide and carbon dioxide. The energy used for the decomposition of calcium carbonate is y kJ. The balanced chemical equation for the reaction is a. CaCO3(s) → CaO(s) + CO2(g) ΔH = +y kJ b. 2CaCO3 (s) → 2CaO(s) + 2C(s) + 2O2(g) ΔH = +2y kJ c. CaCO3(s) → CaO(s) + CO2(g) ΔH = –y kJ d. 2CaCO3(s) → 2CaO + 2CO2(g) ΔH = –2y kJ e. none of the above
The common fertilizer NH,N0;(s), can explosively decompose according to the following reaction. What is the heat released when 80.06 g of NH,NO;(s) explodes? Molar mass of NH,NO:(s)= 80.06 g/mol. 28. 2 NH,NO3(s) → 2 N2(g) + O2(g)+4 H,O (g) AH = -236.15 kJ -472.3 kJ A) B) -236.15 kJ -118.08 kJ D) -59.04 kJ
Consider the following reaction: 2Mg(s)+O2(g)⟶2MgO(s) ΔH∘=−1203 kJ What mass (in grams) of magnesium must be combusted in order to generate 150.0 kJ of heat?
The standard state of carbon is graphite. ΔH°f,diamond is +1.896 kJ/mol. Diamonds are normally weighed in units of carats, where 1 carat = 0.200 g Determine the standard enthalpy of the reaction for the conversion of a 3.61 -carat diamond into an equivalent mass of graphite.
How much heat (in kJ) will be released (AH) if 0.4501 mol of NH3 are mixed with 0.200 mol of O, in the following chemical reaction? 4 NH3 (g) + O2 (g) → 2 N‚H4 (g) + 2 H,O (g) AH° = -286 kJ/mol
Acetylene is used in welding torches because it has a high heat of combustion. When 2.00 of acetylene burns with excess oxygen, it releases 40.8 KJ of energy. What is the molar energy of combustion of acetylene?
2Al(s) + 3Cl2(g) ----à 2AlCl3(s); H = –1390.81 kJ How much heat is produced/required when 10.0 g AlCl3 forms?
6
How many moles of butane, C4H10(l), must be burned to produce 234 kJ of heat under standard state conditions? (The heat of combustion for butane is −2855.7 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).
6
*ONLY THE SECOND PART*