Other Chemistry Answers

The industrial solvent carbon disulfide can be made from the reaction between methane and hydrogen sulfide at elevated temperatures using the following reaction gas-phase reaction: 

2H2S+CH4->CS2+4H2

a. Compute the equilibrium constant for this reaction from 500C to 800C. 

b. Starting with equal number of moles of H2S and CH4, compute the equilibrium compositions of all components in the reaction at 1 bar and over the temperature range of part (a).

c. Repeat the calculation of part (b) for a pressure of 10 bar. Ideal gas mixture behavior may be assumed at this pressure at these high temperatures

Write the balanced chemical equation for the complete combustion of gaseous pentane (C₅H₁₂) and then use bond dissociation energy data to calculate the enthalpy change for this reaction. Assume all reactants and products are in the gaseous state. Finally, state whether the reaction is endothermic or exothermic

A calorimeter that contains 3.6 L of water is used to measure the enthalpy of solution for 45 g of KOH. Calculate the molar enthalpy of solution that is associated with the reaction if the temperature of the water changes from 25.5 °C to 20.7 °C. [The molar mass of KOH is 56.10 g/mol] 

For the thermochemical reaction: C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l) ΔH = -1367.1 kJ. Draw the potential energy diagram that illustrates the enthalpy change in this reaction and state whether the reaction is endothermic or exothermic.