y.omytitehview assignmentProblemID-94281045 bsPlus Homework 4Exercise 12.25 Cour

Question

y.omytitehview assignmentProblemID-94281045 bsPlus Homework 4Exercise 12.25 Courses « previous | 20 of 25 I next » urse Home llabus ssignments Exercise 12.25 You may want to reference ( Part A page) Section 12.1 while completing this problem. cores ourse Tools eText Study Area How many liters of CH4(9), measured at 24.0 °C and Aconti H-_8.90 x 102 kJ mol 1 CH4. For H2O(1) at 100 oC, d0.958 g cm 3 and AnpH--40.7 kJ mol Express your answer in liters to three significant figures. 772 mmHg, must be burned to provide the heat needed to vaporize 3.88 L of water at 100 °C? User Settings SubmitMy Answers Give up eovide Feedback Continue Continue d, TUR 10.12.2017 8 3 4 S 5 6

Explanation / Answer

Given that water = 3.88 L

mass of water at 100 0C = 3.88 L * density of water

                        = 3.88 L * 0.958 g/(10^-3L) ( since 1000 cm^3 = 1L)

mass of Water at 100 0C = 3717.04 g

number of moles of water = 3717.04/18 = 206.5 moles

for 1 mole of water dH vap = 40.7 kJ

for 206.5 moles of water dH vap = 40.7 * 206.5 = 8404.55 kJ

from the data 1 mole of CH4 on combustion produces 8.9 * 10^2 kJ energy

890 kJ energy requires 1 mole of CH4

8404.55 kJ energy requires 1/890*8404.55 moles of CH4

                          = 9.4433 moles of CH4

according to ideal gas equation,

PV = nRT

772/760 * V = 9.4433 * 0.0821 * (24+273.15)

V = volume of CH4 = 226.7979 L required.

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