Brunette

20.0 mL of a 0.125 M solution of potassium iodide is added to 15.0 mL of a 0.235 M solution of lead (II) nitrate. A reaction occurs via the balanced equation below: 2KI(aq)+ Pb(NO3)2(aq) --> 2KNO3(aq) +PBI2(ppt) How much product can theoretically be produ...

Determine the melting point of an aqueous solution containing 115 mg of saccharin (C7H5O3NS)added to 1.00 mL of water (density of water=1.00 g/mL, Kt=1.86 C/m)

Compound: Concentration: Measured deltaT LiCl 6.00 g/kg 0.492 deg C HCl 4.00 g/kg 0.389 deg C NaCl 6.00 g/kg 0.356 deg C Determine the value of the vant hoff factor for each salt for the experimentally measured delta T value. (kf=1.86) I have tried to fig...

The following reation has the following standard thermodynamic parameters: delta H= -33.6 kJ/mol delta S= -59.8 J/(mol*K). C(g) + D(g) --> E(g) Calculate the temperature at which the reaction becomes nonspontaneous.

at high temperatures, ammonia decomposes to N2 and H2. 2 NH3(g)--> N2 (g) + 3H2(g) Delta H for the reaction is positive and delta S is positive. Estimate the temperature at which this reaction becomes spontaneous

Predict the boiling point of the following compound using Trouton's Rule: Heat of vaporization/Tb= 80 J/K Carbon tetrachloride (CCl4) = ?? degrees Celsius

Cl2O2 (g)---> 2ClO (g) Time [Cl2O2] (M) 0....... 6.60*10^-8 172..... 5.68*10^-8 345..... 4.89*10^-8 517..... 4.21*10^-8 690..... 3.62*10^-8 862..... 3.12*10^-8 Determine the value of the first-order rate constant. For this question, you need to graph it o...

Values of the rate constant for the decomposition of N2O5 at four different temperatures are as follows: T(K) k(s^-1) 658....2.14*10^5 673....3.23*10^5 688....4.81*10^5 703....7.03*10^5 The activation energy is 1.02*10^2 kJ/mol. Calculate the value of the...

Given the balanced equation for the decomposition of INO, and the rate of disappearance of INO, write the expressions for the rates of appearance of I2 and NO 2INO(g) ---> I2(g) + 2NO(g) Reactant: Product(I2): Product(NO): -∆[INO]/2∆t = ??/?? = ??/??

The equilibrium constant Kc for the reaction C <--> D + E is 7.90 * 10^-5. The initial composition of the reaction mixture is [C]=[D]=[E]=1.10*10^-3. What is the equilibrium concentrations of C, D, and E? C=? D=? E=?

How much NaOH (g) would you need to dissolve in water in order to prepare 2.75 L of a NaOH solution in which [OH-]= 0.50 M?

The average pH of open ocean water is 8.1. What is the maximum value of [Fe3+] in pH 8.1 seawater if the Ksp of Fe(OH)3 is 1.1*10^-36?

The average pH of open ocean water is 8.1. What is the maximum value of [Fe3+] in pH 8.1 seawater if the Ksp of Fe(OH)3 is 1.1*10^-36? chemistry - DrBob222, Friday, December 7, 2012 at 10:14pm Fe(OH)3 ==> Fe^3+ + 3OH^- pH = 8.1 pH + pOH = pKw = 14 Therefo...

thank you so much!

I did this and the database said the answer was wrong: (213.8 + 70.0) - (186.2 + 2*205.0)= -312.4 j/K*mol. Am I missing something?

Thank you!

I found the answer for carbon tetrachloride. I just need to find it for n-butane (C4H10) and ethanol and the database is saying the answers are wrong. I don't understand why if the format is the same as the carbon tetrachloride

nevermind, I got it. I must have been putting the numbers in wrong or something. :)

U(s) + 3F2(g) ---> UF6(g)

I keep trying that and it is saying that I have the wrong answer. here is my work: slope: -1.19*10^4 y-intercept= 30.439 Ea: -(-1.19*10^4 K) *(8.314J/moK)= 9.89*10^4 J/mol A= e^30.439= 1.65*10^13 (1.65*10^13) e^-(9.89*10^4J/mol/8.314*300 K)= 9.98*10^-5 I...

Nevermind. I figured it out.

Nevermind. I figured it out.