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Consider the following reaction at equilibrium.  What effect will increasing the temperature have on the system?             Fe3O4 (s) + CO(g)  ⇌  3 FeO(s) + CO2 (g)     ΔH°=  +35.9 kJ

Assign the appropriate labels to the phase diagram shown below:

Consider a reaction that has a positive ΔH and a positive ΔS.  Which of the following statements is true?  

How much energy (in kJ) is required to heat 36.0g of H2O from a liquid at 65oC to a gas at 115oC? (molar mass of water = 18.02 g/mol)

Which of the following acids (listed with Ka values) and their conjugate base should be used to form a buffer with a pH of 8.10?   Chapter 17 & 18 equations: pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14.00 Kw = 1 x 10-14 Ka x Kb = Kw = [H3O+][OH-] pKa = -log Ka pH = pKa + log    

Express the equilibrium constant expression for the following reaction:             Pb(NO3)2 (aq) + 2 KCl (aq)   ⇌  PbCl2 (s) + 2 KNO3 (aq)

Lithium crystallizes in a body-centered cubic structure.  What is the coordination number of each atom?

What mass of silver can be plated onto an object in 67 minutes at 8.70 A of current? (molar mass of silver = 107.87 g/mol)             Ag⁺(aq) + e⁻  →  Ag(s)   1 amp = 1 coulomb/sec 1 mol e- = 96,485 coulombs

Calculate ΔG°rxn for the following reaction at 449.0 K:         CH2O(g) + 2 H2(g)  →  CH4(g) + H2O(g)        ΔH°=  -94.9 kJ ΔS°= -224.2 J/K   Chapter 19 Equations:

Commercial grade HCl solutions are typically 39.0% (by mass) HCl in water.  Determine the molarity of the HCl, if the solution has a density of 1.20 g/mL.  (molar mass of HCl = 36.46 g/mol) Chapter 14 Equations: