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September 1, 2014

September 1, 2014

Posted by **maria** on Saturday, October 26, 2013 at 7:41pm.

water. Calculate the mass of natural gas that

would need to be burned to heat the water

for a tub of this size from 56 ◦F to 87 ◦F.

Assume that the natural gas is pure methane

(CH4) and that the products of combustion

are carbon dioxide and water (liquid).

Answer in units of g

2nd part

What volume of natural gas does this correspond to at 30◦C and 1 atm?

Answer in units of L

- chemistry -
**DrBob222**, Saturday, October 26, 2013 at 8:30pma.

1. Convert F to C. Convert 106 gallons H2O to L, assume density of 1.0 g/mL and convert L to grams.

2. Calculate q = heat required to heat the water as described.

q = mass H2O x specific heat H2O x (Tfinal - Tinitial).

3. Write and balance the equation for the combustion of CH4.

CH4 + 2O2 ==> CO2 + 2H2O

4. Calculate heat of combustion.

dHfrxn from step 2 = (n*dHf products) - (n*dHf reactants). Call this dHrxn

5. dHrxn in kJ/16g CH4 x # g CH4 = q

Solve for #g CH4

Check my thinking.

b.

Use PV = nRT and solve for V in L. You will need to plug in for n; remember n = grams/molar mass. You know g and molar mass so you can calculate n and obtain V from there.

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