1 out of 3 attempts Enter your answer in the provided box. A gas company in Mass

Question

1 out of 3 attempts Enter your answer in the provided box. A gas company in Massachusetts charges S1.10 for 15.0 f of natural gas (CH,) measured at 20.0°C and 1.00 atm. Calculate the cost of heating 2.00 x 16 mL of water (enough to make a cup of coffee or tea) from 20.0°C to 100.0 °C, Assume that only 50.0% of the heat generated by the combustion is used to heat the water; the rest of the heat is lost to the surroundings. Assume that the products of the combustion of methane areCO2(g) and H200). Report your answer to the correct number of significant figures.

Explanation / Answer

Heat requirement:

Q = m*C*dT

mass = D*V = 200 mL * 1g/mL = 200 g

Q = 200*4.184*(100) = 83680 J

then, only 50% is used, therefore

Qrequired to burn = 83680 / 50% = 167360 J required from methane

enthalpy of combustion for methane = 882.0 kJ/mol = 882000 J/mol

moles of methane = Qrequired /Enthalpy of comb = 167360/882000 = 0.189750 mol of CH4

now..

get volume

PV = nRT

V =nRT/P

V = (0.189750)(0.082)(20+273)/1 = 4.558 Liters

change to ft3

V = 4.558 L * 0.0353147 ft3/L = 0.1609 ft3 required to burn

15 ft3 = 1.1 $

0.1609 ft3 = x

x = 0.1609*1.1/15

x = 0.01179

sig fig ---> 3

0.0118 $

nearest wil lbe 0.01 $

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