8) Consider the apparatus pictured below, which consists of two containers separated by a valve. C,H;N(g) O2(g) 419 mL 285 mL 591 torr 1766 torr The valve is opened and the gases react as follows (note that the temperature is high enough that the water is produced as a gas): 4 C2H;N(g) + 15 O2(g) → 8 CO2(g) + 14 H20(g) + 2 N2(g) What will be the total pressure in the apparatus when the reaction has gone to completion? Assume that the temperature does not change.

8) Consider the apparatus pictured below, which consists of two containers separated by a valve. C,H;N(g) O2(g) 419 mL 285 mL 591 torr 1766 torr The valve is opened and the gases react as follows (note that the temperature is high enough that the water is produced as a gas): 4 C2H;N(g) + 15 O2(g) → 8 CO2(g) + 14 H20(g) + 2 N2(g) What will be the total pressure in the apparatus when the reaction has gone to completion? Assume that the temperature does not change.

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...

See similar textbooks

Similar questions

etermine the total volume of all gases formed when 75.0 mL an explosive (C3H5(NO3)3 , d = 1.60 g/mL, molar mass = 227.10 g/mol) reacts according to the following reaction. Assume room temperature and pressure conditions. 4 C3H5(NO3)3(l) → 6 N2(g) + O2(g) + 12 CO2(g) + 10 H2O(g)
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4595 L of hydrogen gas at STP, heat the mixture to run the reaction, then isolate the ammonia from the reaction mixture. What volume of NH, in liters, measured at STP, would be produced? Assume the reaction goes to completion. N₂ (g) + 3 H₂(g) → 2 NH, (g)
The Haber Process synthesizes ammonia at elevated temperatures and pressures. Suppose you combine 1580 L of nitrogen gas and 4240 L of hydrogen gas at STP, heat the mixture to run the reaction, then separate the ammonia from the reaction mixture. What volume of reactant, measured at STP, is left over? Assume the reaction goes to completion. N₂ (g) + 3 H₂ (g) → 2 NH₃ (g)
Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. 2 Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 51.0 mL. g x10 X 歐 Sketch of a gas-collection apparatus S collected gas Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about 2 the reaction conditions and the nature of the gases. water chemical reaction
A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)
Please answer questions 1-3 Please refer to the picture below:
SF6 can be synthesized by the reaction: SO2(g) + 3 F2(g) → SF6(g) + O2(g)A 1.25-L reaction vessel, initially at 26°C, contains sulfur dioxide gas at a partial pressure of 184 mmHg and fluorine gas at a partial pressure of 511 mmHg. Identify the limiting reactant and determine the theoretical yield of SF6 in grams.
A sample of gas contains 0.1100 mol of CH4 (9) and 0.1100 mol of H₂O(g) and occupies a volume of 13.1 L. The following reaction takes place: CH4 (9) + H₂O(g) → 3H₂(g) + CO(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant. Volume =
Nitesh
10
A sample of Cl2 with a pressure of 1.84 atm and a volume of 290 mL is allowed to react with excess Br2 at 182 °C. Br2 (g) +Cl2 (g) --> 2BrCl (g) Calculate the pressure of the BrCl produced in the reaction if it is transferred to a 2.16-L flask and cooled to 32 °C