Calculate the change in enthalpy (amount of heat at constant pressure) when a mole of iodine goes from 300 K to 500 K under the pressure of one atmosphere. We give: the molar heat capacities of pure bodies: Cp (I2, solid) =22.6 J/mol K, Cp (I2, liquid) = 81.6 J/mol K Cp (I2, gas) = 37.7 J/mol K, ΔH°v(I2) at 457K = 25.52 kJ/mol, ΔH°F (I2) at 387K = 15.65 KJ/mol

An ideal gas has a gas constant R = 0.3 kJ/kg-K and a constant-volume specific heat Cv = 0.7 kJ/kg-K. If the gas has a temperature change of 100 degrees C, what is the change in enthalpy?Question 2Select one:a.30 kJ/kgb.70 kJ/kgc.100 kJ/kgd.insufficient information to determine

The molar specific heat at constant volume of an ideal gas is equal to 2.5 times the universal gas constant (8.314 J/mol.K). When the temperature increases by 100k, the change in molar specific enthalpy is ___ J/mol.:

The vapor pressure of solid iodine at 25°C is 1.42torr. Calculate the vapor pressure in mmHg and atm. Round each of your answers to 3 significant digits.mmHgatm

(ii) Show that the heat energy change, Q, in the student’s experiment is about 1100 J.[for the mixture, c = 4.2 J/g/°C][massof1.0 cm 3of mixture = 1.0 g] (3)(iii) The student uses 0.020 mol of potassium hydroxide in his experiment.Calculate the enthalpy change (ΔH) in kJ/mol, for 1.0 mol of potassium hydroxide.Include a sign in your answer.

Some lipids contains carbon to carbon double bonds.Given the bond dissociation energies in the table, calculate the enthalpy change when one mole of hydrogen is added across one double bond. A.+1520 kJ/molB.-1520 kJ/molC.+120 kJ/molD.-120 kJ/mol