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CHE330 Study Guide - Quiz Guide: Ideal Gas, Exhaust Gas

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School
University of Waterloo
Department
Chemical Engineering
Course
CHE330
Professor
Yi Feng

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Document Summary

The heat capacity of a substance is represented by the following equation: Cp = a + b t + c t2. Show that the error resulting when h is assumed to be equal to the cp evaluated at arithmetic mean of the initial and final temperatures is. P v1. 55 = constant and the molar heat capacity of the gas is given by. Cp/r = 3. 30 + 0. 63 10-3 t (t in k) Determine the final pressure and the heat transferred during the process: hydrocarbon fuel can be produced from methanol by reactions such as the following, which yields 1-hexene: 6 ch3oh (g) c6h12 (g) + 6 h2o (g) Compare the standard heat of combustion at 25 c of 6 mol ch3oh (g) with the standard heat of combustion at 25 c of 1 mol c6h12 (g), reaction products in both cases being co2 (g) and h2o (g).

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Related Questions

The molar heat capacity C P,m of SO 2 (g) is described by the following equation over the range 300 K < T < 1700 K :
C P,m R = 3.093+6.967×10^−3 T/K
−45.81×10^−7 T^2/K^2 +1.035×10^−9 T^3/K^3
In this equation, T is the absolute temperature in kelvin. The ratios T^n /K^n ensure that C P,m has the correct dimension. 1.40 moles of SO 2 (g) is heated from 28.0 ∘ C to 1.10×103 ∘ C at a constant pressure of 1 bar . Solve for calculate ΔH,q ,ΔU and w.

Physical Chemistry!

Please show steps/explain clearly!

EDIT: Delta U is change in internal energy.

An example: o oThe temperatures before mixing: NaOH solution Tb = 22.72 C o HCl solution Ta = 22.48 C.

The average temperature before mixing is: Ti = (Ta+ Tb)/2 = 22.60 C.To calculate the heat capacity of the calorimeter use Equation 2.

1. In this experiment you will measure the heat capacity of a calorimeter by mixing 50. mL of 1.0 M HCl solution with 50. mL of 1.0 M NaOH solution in the calorimeter. The heat capacity of the calorimeter is expected to be within the range 0 and 100. J/K.

a) At what temperature difference, ?T, does the heat capacity of the calorimeter become larger than 100. J/K?

b) At what temperature difference, ?T, does the heat capacity of the calorimeter become negative?

2. Under what temperature conditions (low T, high T, all T, nonspontaneous at all T) would this reaction occur spontaneously? Explain.