Given the following heat of formation values, calculate the heat of reaction for the following:   C3H8(g) + O2(g) → CO2(g) + H2O(l).   ΔHf value in kJ/mol for C3H8(g) is −103.8, for O2(g) is 0, for CO2(g) is −393.5, and for H2O(l) is −285.8.    3.613 × 102 kJ   1.413 × 102 kJ   −2.220 × 103 kJ   −5.755 × 102 kJ

a) the foul odor of rancid butter is due largely to butanoic acid, a compound contaning oxygen, hyrdrogen and carbon. Combustion analysis of a 4.30g sample of butyric acid produced 8.59g CO2 and 3.52 g H2O. Determine the empircal formula for butyric acid.  b) a colourless liquid has a composition of 84.1% carbon and 15.9% hydorgen by mass. Determine the empirical formula. Also, assuming the molar mass of this compound is 114.2 g/mol, determine the molecular formula of this compound.

This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Based of the table (picture): A. Suppose the ionization enthalpy of M were bigger and the heat of sublimation of M were smaller. Would MX be more or less stable?

Calculate the amount of heat generated (in kJ) from 0.100 g of hydrogen reacting with 0.600 g of oxygen to form water.  242 kJ of heat is released per one mole of water.

Draw the Lewis structure for the following:

What is the lewis structure for SiO2?

Identify the type of reaction shown by the equation: H2O(g)  +  C(s)  →  CO(g)  +  H2(g)

Write a brief paragraph describing the molecule octane (C8H18) and the important function that it serves.

Use the following data to calculate the enthalpy change for the following reaction:  2Na(s) + O2(g) -> Na2O(s) Quantity Magnitude (kJ/mol) Ionization energy of Na(g) 495 Electron affinity of O(g) for 2e 603 Vaporization energy of Na(s) 109 Bond energy of O2(g) 499 Lattice energy for Na2O(s) –2,477

Sodium hydrogen sulfate is used as a cleaning agent and as a flux (a substance that promotes the fusing of metals and prevents the formation of oxides). One of the ways in which sodium hydrogen sulfate is manufactured is by reacting sodium dichromate, Na2Cr2O7, with sulfuric acid. This process also forms water and chromium(VI) oxide, CrO3. Write a balanced equation for this reaction. (You do not need to include states.) How many kilograms of sodium dichromate, Na2Cr2O7, are necessary to produce 130.4 kg of sodium hydrogen sulfate? How many kilograms of chromium(VI) oxide are formed when 130.4 kg of sodium hydrogen sulfate is made? What is the minimum volume of 18.0 M H2SO4 solution necessary to react with 874.0 kg of sodium dichromate? What is the maximum mass of sodium hydrogen sulfate, NaHSO4, that can be formed from the reaction of 874.0 kg of sodium dichromate with 400.0 L of 18.0 M H2SO4?