Recitation 3: Solutions | Answer Key - Edubirdie

University:
Massachusetts Institute of Technology
Course:
3.00 | Thermodynamics of Materials
Academic year:

2019
Views:

497

Pages:

2
Author:

Molly Hanson

Recitation: 3 1. One gram of nitrogen is contained in a constant volume tank at low pressure. Assuming nitrogen to be an ideal gas, calculate the amount of heat required to rise its temperature from 300 to 1000K. For nitrogen C = 6.529 +1.250210-37 (in cal/(gram.mol)K. (hint: use the relation C,C,R) For constant volume process there is no work done and the first law implies AQ = AU. Since nitrogen is taken to be an ideal gas والام 7 AU = CdT To get C, we use the relation C-CR. ΔΩ (where R 1.987 cal/(g.mol)K). Substituing back, 1000 300 (6.529-1.987+0.00125 + T)dT AQ = Integrating ΔΩ 4.542(1000-300)+0.00125/2(10002-3002) = 3748cal (C-R)JT In joules, 3748 cal 15,682 Joules. 2. Find the change in the internal energy of a pound of O₂ (assume ideal gas) heated from 20C to 30C at constant pressure of latm. Calculate heat capacity at constant volume and internal energy of the system. (specific heat capacity of O2 = 0.231 cal/g. K). One pound of O, equals 453.6 gms of O2. Using the First law of thermodynamics, dU =dQ+dW PAV = NRAT and from the definition of C, (C,=p) CAT = Q From the first law, the change in internal energy is given by AU CAT-RAT Remember that the specific heat capacity is given in 'per gram' units. Since O, is a diatomic molecule, one mole of O₂ weighs 32 gms. plugging these conversions in the above equation would lead to SU 766.5 calories.

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