he chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 4 2 CH1 (g) + 3 Cl2 (g) 2 CH3 Cl(g) + 2HCl(g) + 2 C[ (g) Suppose that a chemist combines 163 mL of methane and 659 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K . If the reaction reaches 86.7% completion, what is the total pressure in the flask? Ptotal = What is the partial pressure of CH1 ? PCH4 = What is the partial pressure of Cl2 ? Pc12 = atm atm atm

he chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 4 2 CH1 (g) + 3 Cl2 (g) 2 CH3 Cl(g) + 2HCl(g) + 2 C[ (g) Suppose that a chemist combines 163 mL of methane and 659 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K . If the reaction reaches 86.7% completion, what is the total pressure in the flask? Ptotal = What is the partial pressure of CH1 ? PCH4 = What is the partial pressure of Cl2 ? Pc12 = atm atm atm

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...

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A small amount of oxygen gas may be prepared in the laboratory by the decomposition of potassium chlorate, KClO3, according to the following equation: 2KClO3(s)  2KCl(s) + 3O2(g) A 1.54-g sample of KClO3 is completely decomposed and the oxygen gas produced is collected over water at 25oC and at a total pressure of 757.0 torrs. (a) If the vapor pressure of water at 25oC is 23.8 torr, what is the partial pressure of O2 collected? (b) How many milliliters (mL) of O2 gas are collected under the stated condition? What is the volume of O2 gas if collected at STP?
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The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH,(g)+3Cl,(g)–2CH,CI(g)+2HCI(g)+2CI(g) Suppose that a chemist combines 257 mL of methane and 599 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 87.2% completion, (a) What is the partial pressure of CH;CI? (b) What is the partial pressure of HCI? (c) What is the partial pressure of CI? (d) What is the partial pressure of Cl,? (e) What is the partial pressure of CH,? (f) What is the total pressure?
What volume of carbon dioxide (in L) will be produced from the complete combustion of 370.2 g of octane? Assume the carbon dioxide is at 27.67ºC and 0.872 atm. Give your answer to 3 sig figs. 2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)
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A sample of gas contains 0.150 mol of N₂(g) and 0.300 mol of H₂(g) and occupies a volume of 21.4 L. The following reaction takes place: N₂(g) + 2H₂(g)-N₂H4(9) Calculate the volume of the sample after the reaction takes place (assume temperature and pressure are constant).
The chlorination of methane occurs in a number of steps that results in the formation of chloromethane and hydrogen chloride. The overall reaction is 2CH, (g) +3 Cl, () 2CH,CI(g) + 2 HCI(g) + 2CI (g) Suppose that a chemist combines 273 mL of methane and 689 mL of chlorine at STP in a 2.00 L flask. The flask is then allowed to stand at 298 K. If the reaction reaches 75.0% completion, what is the total pressure in the flask? Pictal = atm What is the partial pressure of CH,? Pon, = atm What is the partial pressure of Cl, ?
A sample of gas contains 0.1700 mol of NH,(g) and 0.2125 mol of O,(g) and occupies a volume of 21.8 L. The following reaction takes place: 4NH3(g) + 502(g) 4NO(g) + 6H,O(g) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.