please i need the answer step by step for self test 2c.7 the anwer is -163kjmol-

Question

please i need the answer step by step for self test 2c.7 the anwer is -163kjmol-1 But they did mot show the steps ..

Example 2C.2 Using Kirchhoff's law The standard enthalpy of formation of H,O(g) at 298 K is -241.82k) mol-. Estimate its value at 100°C given the fol- lowing values of the molar heat capacities at constant pres sure: H,O(g): 33.58 J K-1 mol-, H2(g): 28.84 JK- mol; 0,(g): 29.37J-mol-1. Assume that the heat capacities are independ ent of temperature. Method when ,C is independent of temperature in the range T, to T2, the integral in eqn 2C.7a evaluates to (T-T )4cf. Therefore, Figure 2C.3 and a refere metal heat s to maintain To proceed, write the chemical equation, identify the stoichio- temperatur metric coefficients, and calculate ,C)from the data. Answer The reaction is H,(g)+10,(8H,og), so and is the supply that reference co If no ph temperatur --9.94JK- mol" It then follows that 4,H9(373 K)=-24 1.82 kJ mol-l +(75 K) independer chemical o where qpes Self-test 2C.7 Estimate the standard enthalpy of formation of attain the sa trol. The q Answer-163 kJ mol change in t x(9.94] K-"mol-1-242.6 kJ mol-l cyclohexane, C, H,2(1), at 400 K from the data in Table 2C.6 Cp duringt 2C4 Experimental techniques The classic marized in been made that allow measurement P.ex ic tool of thermochemistry is the calorimeter, as sum, where P. n Topic 2B. However, technological advances have equalize the s to he made

Explanation / Answer

2c.7 cyclohexane is prepared by hydrogenation of benzene.

I don’t have the access of table 2c.6, so assuming

DelH formation at 298k for cyclohexane (l)= -156kJ/mol

Cp = 154.9J/mol/k

DelH formation at 400k =-156+154.9*(298-400)*10-3

= -172kJ/mol

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