Determine the final pressure of the system (i.e. after the reaction has occurred) if 45.2 grams of gaseous nitrogen are allowed to react with 252 grams of gaseous chlorine to produce liquid nitrogen trichloride according to the reaction below. The reaction takes place in a 11.5 L container at a temperature of 319 K. Assume that the liquid has 0 vapor pressure and takes up a negligible amount of volume. Report the value of your pressure in atm (do not include units in the answer field). N2 (g) + 3 Cl2 (g) -> 2 NCI3 (1)

Determine the final pressure of the system (i.e. after the reaction has occurred) if 45.2 grams of gaseous nitrogen are allowed to react with 252 grams of gaseous chlorine to produce liquid nitrogen trichloride according to the reaction below. The reaction takes place in a 11.5 L container at a temperature of 319 K. Assume that the liquid has 0 vapor pressure and takes up a negligible amount of volume. Report the value of your pressure in atm (do not include units in the answer field). N2 (g) + 3 Cl2 (g) -> 2 NCI3 (1)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter10: Solids, Liquids, And Phase Transitions

Section: Chapter Questions

Problem 38P

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