Describe the relationship between gas volume and Kelvin temperature when the pressure is constant (Charles’s law).

Use the following enthalpies of formations (∆Hof): C6H6(l) H2O(g) CO2(g) ∆Hof 49 kJ/mol -242 kJ/mol -394 kJ/mol to calculate the standard enthalpy of reaction (∆Horxn) for the following reaction: 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(g) ∆Horxn = ?

Calculate the pressure of 2520 moles of hydrogen gas stored at 27.0oC in the 180. L storage tank of modern hydrogen-powered car.

Calculate the enthalpy change for the following reaction: 2C2H4(g) + H2O(l) → C4H9OH(l) ∆H = ? Given the following reactions and their ∆H values: 2CO2(g) + 2H2O(l) → C2H4(g) + 3O2(g) ∆H = 1411.1 kJ C4H9OH(l) + 6O2(g) → 4CO2(g) + 5H2O(l) ∆H = -1534.7 kJ

What is the final volume of a sample of gas initially occupying 7.50 L at 10.0oC and 1.00 atm pressure after its pressure is increased to 1.20 atm and its temperature is increased to 37.0oC ?

Predict whether the following compounds are soluble or insoluble in water. a) Pb(NO3)2  – [a] b) AgI – [b] c) NH4Cl – [c]

Calculate the enthalpy change for the following reaction: 2Fe(s) + 3CO2(g) → Fe2O3(s) + 3CO(g) ∆H = ? Given the following reactions and their ∆H values: 4Fe(s) + 3O2(g) → 2Fe2O3(s) ∆H = -1648.4 kJ 2CO(g) + O2(g) → 2CO2(g) ∆H = -565.4 kJ

Predict whether the following compounds are soluble or insoluble in water. a) Ca3(PO4)2  – [a] b) Fe(OH)3 – [b] c) NH4Br – [c]

An unknown substance has a mass of 12.9 g. The temperature of the substance increases from 27.1oC to 42.7oC when 89.1 J of heat is added to the substance. Substance Specific Heat (J/g·°C) Lead 0.130 Silver 0.240 Copper 0.385 Iron 0.442 Aluminum 0.892 Water 4.184   a) What is the specific heat of the unknown substance ? [a] J/goC b) Based on the substances shown on the table above, what is the most likely identity of the unknown substance ?[b]

Select the coefficients that should be placed in front of each molecule, from left to right, to balance the following reaction. C2H6(g) + O2(g) → CO2(g) + H2O(g)