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One of the commercial uses of sulfuric acid is in the production of calcium sulfate and phosphoric acid. If 23.7 g of Ca3(PO4)2 reacts with an excess of H₂SO4, what is the percent yield if 13.4 g of H3PO4 are formed in the following UNBALANCED chemical equation? Ca3(PO4)2 (S) + H₂SO4 (aq) → H3PO4 (aq) + CaSO4 (aq)

One of the commercial uses of sulfuric acid is in the production of calcium sulfate and phosphoric acid. If 23.7 g of Ca3(PO4)2 reacts with an excess of H₂SO4, what is the percent yield if 13.4 g of H3PO4 are formed in the following UNBALANCED chemical equation? Ca3(PO4)2 (S) + H₂SO4 (aq) → H3PO4 (aq) + CaSO4 (aq)

Chemistry
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...
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One of the commercial uses of sulfuric acid is the production of calcium sulfate and phosphoric acid if 23.7g if Ca3(PO4) reacts with an excess of H2SO4 what is the percent yield if 13.4g of H3PO4 are formed in the following unbalanced chemical equation Ca3(PO4)2(s)+H2SO4(aq)=H3PO(aq)+CaSO4(aq)
One of the commercial uses of sulfuric acid is in the production of calcium sulfate and phosphoric acid. If 23.7 g of Ca3(PO4)2 reacts with an excess of H₂SO4, what is the percent yield if 13.4 g of H3PO4 are formed in the following UNBALANCED chemical equation? CA3(PO4)2 (S) + H₂SO4 (aq) → H3PO4 (aq) + CaSO4 (aq)
Transcribed Image Text:One of the commercial uses of sulfuric acid is in the production of calcium sulfate and phosphoric acid. If 23.7 g of Ca3(PO4)2 reacts with an excess of H₂SO4, what is the percent yield if 13.4 g of H3PO4 are formed in the following UNBALANCED chemical equation? CA3(PO4)2 (S) + H₂SO4 (aq) → H3PO4 (aq) + CaSO4 (aq)
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