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When organic matter decomposes under oxygen-free (anaerobic) conditions, methane is one of the products. Thus, enormous deposits of natural gas, which is almost entirely methane, serve as a major source of fuel for home and industry.
(c) What volume (in ft³) of natural gas, measured at STP, is required to heat 1.00 qt of water from 25.0°C to 100.0°C (d of H₂O = 1.00 g/mL; d of CH₄ at STP = 0.72 g/L)?

Respuesta :

shaikhmohd0119

0.29  ft³ volume of natural gas, measured at STP, is required to heat 1.00 qt of water from 25.0°C to 100.0°C

Now,

 Here , Substitute 25.0°C as initial temperature and 100.0°C as final temperature.

 In order to calculate the change in temperature,

We have,

  ΔT= 100.0°C - 25.0°C

       = 75°C

Now,

  substitute 1 as a mass , 4.184 J/g°C as the specific heat of the water, 75°C as the change in temperature and 802kJ/mol as q in equation to calculate mass of methane as shown,

 Hence ,

   Mass of methane = 1qt × L/1.05791 × 1ml/10⁻³L × 1g/1ml × 4.1843/g°C   ×75°C × 1 kJ/ 10³ J × 1 mol/803 kJ

        Mass of methane= 16.04g/mol

Now,

 Moles of methane = 0.370 moles

 Molecular mass of methane = 16.04g/mol

Now,

 mass of methane = 16.04 × 0.370

                               = 5.935 g

Now,

 Substitute 5.935 g as mass and 0.72  g/L as density in the expression of density to find the volume as shown :

 V (in ft³) = 5.935 × 1/0.72 ×10⁻³/ 1 × 35.3ft³/ 1

  V (in ft³) = 0.290ft³

From the above conclusion we can say that , 0.29  ft³ volume of natural gas, measured at STP, is required to heat 1.00 qt of water from 25.0°C to 100.0°C

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