Consider the reaction between HCl and O2: 4HCl(g)+O2(g)→2H2O(l)+2Cl2(g) When 63.1 g of HCl are allowed to react with 17.2 g of O2, 53.8 g of Cl2 are collected. Determine the theoretical yield of Cl2 and the percent yield for the reaction.

What is the vapor pressure of an ideal solution of ethanol if 1 mile of glycerin is placed in 4 moles of ethanol at 40?C? Pure ethanol has a vapor pressure of 135.3 torr.

Calculate the pH and the pOH of an aqueous solution that is 0.035 M in HCL (aq) and 0.075 M in HBr(aq) at 25^.C.

A chemist has a substance which was either phenol or resorcinol. He puts the substance in a test tube, and puts the test tube in a beakar of boiling water. The substance melted. what was the substance and could you say whether the substance was pure or not

You are investigating the effect of strong base on the solubility of zinc hydroxide, Zn(OH)₂ (s).

(Ksp= 3 x 10^{- 15} for Zn(OH)₂ (s))

You prepare 1.0 L solution of 0.10M NaOH and add excess zinc hydroxide, Zn(OH)₂ (s).

Instead of suppresing the solubility, you observe extra solubility.

Your research advisor tells you that zinc ions react with four hydroxide ions in a solution to form the complex ion Zn(OH)₄^2- (aq).

(K_f = 2 x 10 ¹⁵ for Zn(OH)₄^2- (aq))

Calculate the pH of your solution.

Calculate the pH of a 0.50 M solution of sodium benzoate (NaC₆H₅COO) given that the K_a of benzoic acid (C₆H₅COOH) is 6.50 x 10^-5.

The initial concentrations of Na+ and Cl− in the reaction below are each 0.0843 M. If the initial concentration of NaCl is 0 M and the equilibrium constant is Kc=8.21 under certain conditions, what is the equilibrium concentration of Na+?

NaCl(aq)⇌Na+(aq)+Cl−(aq)

12) Calculate the change in pH when 3.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH3(aq) and 0.100 M in NH4Cl(aq).

delta pH=?

Calculate the change in pH when 3.00 mL of 0.100 M NaOH(aq) is added to the original buffer solution.

delta pH=?

Draw a sketch for the Hydrogen (discrete) spectrum, labeling the lines according to their respective quantum transitions. Also point out in which direction the wavelength increases.

1. Retention time (tR) is a measure of how long a compound is retained on a stationaryphase in column in column chromatography. In TLC, Rf was a measure of how long thecompound was retained on the stationary phase. What is the relationship between tR and Rf?

2. What would be the order of elution if one separated the pigments of spinach on columnchromatography?

3. What if any would you have to change in terms of the mobile phase if you wanted toactually perform the column chromatography in order to separate the pigments of spinachcompare to the one used for the TLC Experiment? Explain.

4. Why is it important to keep the solvent level above the stationary phase? What wouldhappen if one lets the solvent get much lower than the alumina stationary phase?

40.0 mL of 0.10 M HA(aq) was titrated against 0.10 M NaOH(aq). HA (aq) is a weak acid with K_aof 6.3 x 10^-6.

            (a)        Calculate the initial pH of the 0.10 M HA (i.e. before adding NaOH).

            (b)        Calculate the pH at the equivalence point.

1) Calculate scattering particles off of a single crystal of nickel. The Ni lattice spacing is 2.15 x 10-10 m. Compute the angle for the first order diffraction feature assuming you bombard the system with:

a. X-ray photons of energy 18.0 keV.

b. Electrons with kinetic energy 18.0 keV.

c. Neutrons with kinetic energy 18.0 keV.

d. What do you conclude from your results above?

calculate pH from 75 ml of 0.1M CH3COOH and 25 ml of 0.1 M Ca(OH)2

Consider the following reaction:
2NO(g)+O2(g)→2NO2(g)
Estimate ΔG∘ for this reaction at each of the following temperatures and predict whether or not the reaction will be spontaneous. (Assume that ΔH∘ and ΔS∘ do not change too much within the give temperature range.)

A)298 K

B)735 K

C)855 K

50 mL of 0.060 M K₂CrO₄ is mixed with 50 mL of 0.080 M AgNO₃. Calculate the following:

a. The solubility of Ag₂CrO₄ (K_sp = 1.9 X 10^-12) in the solution in moles per liter.

b. The concentrations of the following ions Ag⁺, CrO₄^-2, K⁺, and NO₃^-.