The reaction 8H2(g) + S8(l) 8H2S(g) is run at 125oC and a constant pressure of 12.0

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The reaction 8H2(g) + S8(l) → 8H2S(g) is run at 125oC and a constant pressure of 12.0 atm. Assuming complete reaction, what mass of S8 would be required to produce 6.00 × 102 mL of H2S gas under these conditions?

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General Chemistry

ISBN: 978-1439043998

9th edition

Authors: Darrell Ebbing, Steven D. Gammon

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Question Posted: Mar 01, 2016 03:41 AM

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The reaction 8H2(g) + S8(l) 8H2S(g) is run at 125oC and a constant pressure of 12.0

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The moles of H 2 S gas formed is n 120 ...View the full answer

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