please answer correctly Exercise 7.17 Part B The combustion of methane gas, the

Question

please answer correctly

Exercise 7.17 Part B The combustion of methane gas, the principal constituent of natural gas, is represented by the equation CH4 (g) + 202 (g) CO2 (g) + 2H20 (1) AH890.3 kJ mol 1 What quantity of heat, in kilojoules, is liberated in the complete combustion of 1.55x10 CH4(9), measured at 19.2 °C and 774 mmHg? Express your answer to three significant figures. You may want to reference ( while completing this problem page ) Section 7.1 - 5.63 10 Submit My Answers alhe ip kJ Incorrect; Try Again; 2 attempts remaining Part C If the quantity of heat calculated in part B could be transferred with 100% efficiency to water, what volume of water, in liters, could be heated from 90 to 55.0 °C as a result? Express your answer to three significant figures. ^q. El TUR 22.11.2017 0

Explanation / Answer

B)

we have:

P = 774.0 mm Hg

= (774.0/760) atm

= 1.0184 atm

V = 15500.0 L

T = 19.2 oC

= (19.2+273) K

= 292.2 K

find number of moles using:

P * V = n*R*T

1.0184 atm * 15500 L = n * 0.08206 atm.L/mol.K * 292.2 K

n = 658.3 mol

From reaction,

for 1 mol, |Q| = 890.3 KJ

So,

for 658.3 mol, |Q| = 658.3 * 890.3 KJ

= 5.86*10^5 KJ

Answer: 5.86*10^5 KJ

C)

Q = 5.86*10^5 KJ

specific heat capacity of water,

C = 4.184 KJ/Kg.oC

use:

Q = m*C*(Tf-Ti)

5.86*10^5 KJ = m*4.184 KJ/Kg.oC*(55.0-9.0) oC

m = 3.04*10^3 Kg

since density of water is 1 Kg/L,

volume will be 3.04*10^3 L

Answer: 3.04*10^3 L

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