How many liters of CO2 gas can be produced at 30.0 °C and 1.50 atm from the reaction of 5.00 mol of C3Hg and an excess of O₂ according to the following equation? C3H8 (9) +502 (g) → 3CO2 (g) + 4H₂O(g) View Available Hint(s) Hint 1. General approach to solving the problem First, convert from moles of C3Hg to moles of CO₂ using the mole ratio from the balanced chemical reaction. Then use the ideal gas equation to firm volume of CO₂ using the given temperature and pressure, and the number of moles you calculated in step one. See Section 10.5 (Page 408).
How many liters of CO2 gas can be produced at 30.0 °C and 1.50 atm from the reaction of 5.00 mol of C3Hg and an excess of O₂ according to the following equation? C3H8 (9) +502 (g) → 3CO2 (g) + 4H₂O(g) View Available Hint(s) Hint 1. General approach to solving the problem First, convert from moles of C3Hg to moles of CO₂ using the mole ratio from the balanced chemical reaction. Then use the ideal gas equation to firm volume of CO₂ using the given temperature and pressure, and the number of moles you calculated in step one. See Section 10.5 (Page 408).
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter5: Gases
Section: Chapter Questions
Problem 162CP
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How many liters of CO₂ gas can be produced at 30.0 °C and 1.50 atm from the reaction of 5.00 mol of C3Hg and an excess of O₂ according to the following
equation?
C3Hg (g) +502 (g) → 3CO2 (g) + 4H2O(g)
▾ View Available Hint(s)
▼ Hint 1. General approach to solving the problem
First, convert from moles of C3Hg to moles of CO2 using the mole ratio from the balanced chemical reaction. Then use the ideal gas equation to find
volume of CO₂ using the given temperature and pressure, and the number of moles you calculated in step one. See Section 10.5 (Page 408).
O24.6 L
O249 L
O27.6 L
82.9 L
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