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 andwater react to form acetylene and calcium hydroxide:CaC,(s)+2H,0(9)→C,H,(9)+Ca(OH),(s)In the second step, acetylene, carbon dioxide and water react to form acrylic acid:6C,H,(9)+3 CO,(g)+4H,0(g)→5 CH,CHCO,H(9)Write the net chemical equation for the production of acrylic acid from calcium carbide, water and carbon dioxide. Be sure your equation is balanced.

All atoms of all elements and charges should be balanced in a balanced chemical reaction.

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)+2H,O(9)→C,H,(9)+Ca(OH),(s) In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H,(9)+3 CO,(g)+4H,O(g)→5CH,CHCO,H(9) Write the net chemical equation for the production of acrylic acid from calcium carbide, water and carbon dioxide. Be sure your equation is balanced.

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)+2H,O(9)→C,H,(9)+Ca(OH),(s) In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6C,H,(9)+3 CO,(g)+4H,O(g)→5CH,CHCO,H(9) Write the net chemical equation for the production of acrylic acid from calcium carbide, water and carbon dioxide. Be sure your equation is balanced.

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

There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2 Cu,S(s)+3O,(9)2 Cu,0(s)+2 SO,(9) In the second step, copper(I) oxide and carbon react to form copper and carbon monoxide: Cu,O(s)+C(s)→2 Cu(s)+CO(g) Write the net chemical equation for the production of copper from copper(I) sulfide, oxygen and carbon. Be sure your equation is balanced. ローロ

Consider the reaction below for the combustion of methane (CH4, which is the principal component of natural gas). When natural gas is combusted, heat is given off that can be used to provide warmth in homes as well as to heat water, and it is increasingly used as an alternative to coal for the production of electricity. CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) + q Which of the following statements are correct? The combustion of methane is endothermic, and the sign of ∆Hrxn is negative. The combustion of methane is endothermic, and the sign of ∆Hrxn is positive. The combustion of methane is exothermic, and the sign of ∆Hrxn is positive. The combustion of methane is exothermic, and the sign of ∆Hrxn is negative.
For each chemical reaction listed in the table below, decide whether the highlighted atom is being oxidized or reduced. reaction H₂S(aq) + 2NaOH(aq) → Na₂S(aq) + 2 H₂O(1) FeO(s)+CO(g) → Fe(s) + CO₂(g) CO(g) + H₂O(g) → CO₂(g) + H₂(g) 2 NH3(aq) + H₂SO4(aq) → (NH4)2SO4(aq) highlighted atom is being... oxidized reduced O O O X neither oxidized nor reduced 5
Nitric acid (HNO3) reacts with iodide ions (I-) to form iodine (I2) and nitrogen oxide (NO) in an acidic aqueous solution. Write the balanced equation for this reaction.
Balance the following chemical equation (if necessary):
answeeer
Which of the following is the formation reaction for Na2CO3 (s)? A. 2 Na(s) + C(s, graphite) + 3 O(g) → Na2CO3(s) B. 4 Na(s) + 2 C(s, graphite) + 3 O2(g) → 2 Na2CO3(s) C. 2 Na(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) D. Na2(s) + C(s, graphite) + 1.5 O2(g) → Na2CO3(s) E. 2 Na(g) + C(g) + 1.5 O2(g) → Na2CO3(s)
The compound sodium thiosulfate pentahydrate, Na2S2 O3-5H2O, is important commercially to the photography business as "hypo," because it has the ability to dissolve unreacted silver salts from photographic film during development. Sodium thiosulfate pentahydrate can be produced by boiling elemental sulfur in an aqueous solution of sodium sulfite. S8 (s) + Na2 SO3 (aq) + H2O(1) → Na2 S2 O3-5H2 O(s) (unbalanced) What is the theoretical yield of sodium thiosulfate pentahydrate when 3.25 g of sulfur is boiled with 13.1 g of sodium sulfite? Sodium thiosulfate pentahydrate is very soluble in water. What is the percent yield of the synthesis if a student doing this experiment is able to isolate (collect) only 5.26 g of the product?
15. Kkura found a sulfide ore in the dungeon which she identified to be chalcocite. While waiting for her debut, she read from a journal that grinding and "roasting" (heated strongly with oxygen gas) chalcocite can generate copper (1) oxide, a pigment used to color ceramics. Find the amount of copper(I) oxide she can produce from 53 grams copper(I) sulfide. Cu2S(s) + O2(g) –> Cu2O(s) + SO2(g)
The chemical equations below show reactions similar to those you have met already. One of them is balanced correctly, and three are not. Identify which one is correctly balanced. State why. - 4 Fe (s) + 3 O2 (g) = 2 Fe2O3 (s) - Mg (s) + O2 (g) = 2 MgO (s) - 2 K (s) + 2 O2 (g) = 2 K2O (s) - 2 Na (s) + H2O (l) = 2 NaOH + H2 (g)
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N,(0) + 3 H,(9) → 2 NH,(9) ΔΗ-92. k In the second step, ammonia and oxygen react to form nitric acid and water: NH,(9) + 20,(9) → HNO3(g) + H,O(g) AH=-330. kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen from these reactions. Round your answer to the nearest kJ. ?
Consider the synthesis of ammonia: N2 (g) +3H, (g) 2NH3 (g)