If 9.86 L of gaseous Cl2 measured at STP and 63.2 g of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many milliliters of liquid CCl4 are produced? CS2(l) + 3Cl2(g) → CCl4(l) + S2Cl2(l) Molar Mass (g/mol) Cl2 70.906 CS2 76.143 CCl4 153.82 Density (g/mL) CS2 1.26 CCl4 1.60 Molar Volume (L) 22.4 at STP Gas Constant(L.atm.mol-1.K-1) 0.0821
If 9.86 L of gaseous Cl2 measured at STP and 63.2 g of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many milliliters of liquid CCl4 are produced? CS2(l) + 3Cl2(g) → CCl4(l) + S2Cl2(l) Molar Mass (g/mol) Cl2 70.906 CS2 76.143 CCl4 153.82 Density (g/mL) CS2 1.26 CCl4 1.60 Molar Volume (L) 22.4 at STP Gas Constant(L.atm.mol-1.K-1) 0.0821
Introductory Chemistry: A Foundation
8th Edition
ISBN:9781285199030
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter13: Gases
Section: Chapter Questions
Problem 98QAP
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If 9.86 L of gaseous Cl2 measured at STP and 63.2 g of liquid CS2 are reacted stoichiometrically according to the balanced equation, how many milliliters of liquid CCl4 are produced? |
CS2(l) + 3Cl2(g) → CCl4(l) + S2Cl2(l)
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Gas Constant (L.atm.mol-1.K-1) |
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