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Physical Chemistry

Calculating Kc

Given the amount of reactant in grams in a container at a temperature and amount produced in moles, calculate Kc: A quantity of 6.75 g of SO2Cl2 place in a 2.00 L flask. At 648 K, there is 0.0345 mol of SO2 present. Calculate Kc for the reaction. SO2Cl2(g) f/r SO2(g)+Cl(g)

Acid-base titration; density & specific heat of a solid

1.What data is collected in a titration? 2.How would I be able to find what the volume of 0.10M HCl should be needed to titrate .136 g Na2CO3 according to the reaction equation: Na2CO3(aqueous) +2HCl(aqueous)  2NaCl(aqueous) + H2O(liquid) + CO2(gas) 3.How would I determine the density of a solid using water di

Molarity and Solubility

1) If ZnCO3 (solid) is insoluble in water, but dissolves in excess 6.0 molar HCl (aqueous), how would pull out the proper equation that would support it? 2) How would you go about finding how many mL of 2.00 molar NaOH (Aqueous) solution are required to neutralize 1.858 g of KHC8H4O4 (it's formula weight being 204.22)? An

Reactions within equations and properties of acidity

A reaction occurs for each of the following below. How do you differentiate between the different driving forces? (a driving force can either be the transfer of electrons; the formation of a precipitate, etc.) 2Na(s) + 2H2O(l) --> 2NaOH(aq) + H2 KOH(aq) + HF(aq) --> KF(aq) + H2O(l) NaF(aq) + HCl(aq) --> NaCl(aq) + HF(

Thermodynamics Question

I solved part a of this problem easily. The rest of this problem has me stumped. I already have the solutions to these problems, but it's arriving at these solutions that has made me pull my hair out!

Calculation

Calculate the heat of decomposition for this process at constant pressure and 25o: CaCO3(s) ---> CaO(s) + CO2(g)

Chemistry Based Calculations: Molar Solubility

Hi, I need some assistance with the following questions: 1. Calculate the molar solubility of AgCl in a 1.00L solution containing 10.0g of dissolved CaCl2. 2. Compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH of 9.0.

Electrolyte Concentration and Polarization Potential

I am having some trouble with this question. Question: a) A copper refining cell is operating with an electrolyte which contains 0.05 m Sn2+. At what concentration of Cu2+ will the tin start to plate out in preference to the copper? The cell temperature is 40 degrees Celsius. b) A polarization potential arises from a con

Solubility Constant, Ksp of Reactant

The chemical reaction representing the soluability of AGBr is: AgBr (right and left arrow) Ag^+ +Br^- This can be written as: AgBr+ 1e^- (right arrow) Ag + Br^- Eo=.071 V Ag (right arrow) Ag^+ +1e^- Eo=-.800 Using this data, what is the solubility product constant, Ksp, of AgBr @ 25 Celsius?

Calculating cell potential...

Calculate the cell potential @ T=25 celsius assuming ideal solutions Fe | Fe^2+ (1.43 *10^-5) || Fe^2+ (5.00*10^-4M) | Fe The double line represents a salt bridge. I need detailed description of what they are talking about here - I haven't a clue!!

Rate Law for Proposed Mechanism

Consider the reaction 2NO(g) + O2 ---> 2NO2 (g). The following mechanism has been proposed to explain the experimental rate law: 1. 2NO --> and <-- N2O2 (fast) 2. O2 + N2O2 --> 2NO2 (slow) Give the rate law for the proposed mechanism. If necessary, use the pre-equilibrium assumption to determine an expression for the co

Rate Constant with Temperature Changes

Rearrangement of methyl isonitrile to acetonitrile has activation energy of 25.0 kJ/mol and a rate constant of 8.1*10^-4s-1 @ 80 Celsius. what is the value of the rate constant @ 255.0 celsius?

Half-life of first order process

A reactant undergoes a dissociation reaction A r arrow 2B which follows first order kinetics. The initial concentration of reactant A is .4000 M and after 75.00 hr the concentration of A decreases to 0.0816 M. Determine the half-life of the first order process. There must be a simple equation for this, but my textbook must a

Mathematics of pH Acidity

If 50.0 mL of a 0.1 solution of HOAc (Ka = 1.8 x 10^-5) has been titrated to the equivalence point with 0.1 M NaOH solution, what is the pH of the resulting solution? Please explain the math. Thanks.

Level of pH Acidity

Calculate the pH of a 1.0 M solution of NH4Cl with the following parameter given: Kb=1.8 x 10^-5 for NH3

Balancing a Reaction

Balance the following reactions: Pb(s) + PbO2(s) + H2SO4 --> PbSO4(s) H3AsO4 + Zn(s) --> As + Zn^+2 O3 + NO --> O2 + NO2

Amount of natural gas burned is proportional

nt of natural gas burned is proportional to the amount of oxygen consumed. if 24.0 kg of oxygen is consumed in burning 15.0 kg of natural gas, how much air, which is 23.2% oxygen by weight, is consumed to burn 50.0 kg of natural gas? a. 80.0 kg b. 345 kg c. 31.3 kg d. 135 kg

Only for 103139,103997, 103940, or 103642 only

Only for above OTAs If doing by hand, please write dark onpaper before scanning. Thanks Balance and do total net ionic equations Please Explain math ... __NaCNS +__ KmnO4 +__H2SO4 arrow __K2SO4 + __MnSO4 + __NaCN +__H2O __Cu + __HNO3 __Cu(NO3)2 + __ NO + __H2O __U3O8 +__ H2SO4 arrow __UO2SO4 + __U(SO4)2 + __H20 __B

Only for 103139,103997,, 103940, or 103642 only

Only for above OTAs Balance and do net ionic equation Explain Acidic: __Ag+__NO3^-1__Ag^+1 +__NO __IO4^-1 + __I ^-1 __I2 __Cr2O7-2 + __I-1 ® __Cr+3 + __I2 __P + __NO3^-1 __NO + __H3PO4 __SeO4^-2 +__ Cl^-1 SeO3^-2 + __Cl2 __Cr^+3 + __ClO3^-1 __CrO4^-2 + __Cl^-1 __Br2 arrow __Br^-1 + __BrO3^-1

Oxidation and reduction - arranging reactions in order

I am having trouble with this question: i) A reacts spontaneously with 1 mol/L BNO3, 1 mol/L D(NO3)2 and dilute sulfuric acid. A does not react with 1 mol/L C(NO3)2 ii) B does not react spontaneously with any of the 1 mol/L solutions above or with dilute sulfuric acid. iii) C reacts spontaneously with dilute sulfuri

Explain order

Please explain order: 1.24 = K[4.42]^n [1.00]^m / o.169 = K[2.21]^n [1.00]^m The answer is overall 2nd order- why???

Soluble salts

Please explain which of the following salts is most soluble? CuS(s) Ksp = 8.5 x 10^-45 Ag2S(s) Ksp = 1.6 x 10^-49