Suppose a 3.00 L nickel reaction container filled with 0.0072 M H2 is connected to a 3.00 L container filled with 0.247 M F2. Calculate the molar concentration of H2 at equilibrium.

-Hint, find the equilibrium concentration of HF and F2 (as in the above problem), then use the equilibrium expression to find the hydrogen concentration.

-When you do the limiting reactant calculation you essentially use up all the limiting reactant. So, hydrogen concentration is approximately zero. But, it can't be identically equal to zero or the Keq expression can not be correct. You will find how small it really is.

write the complete mechanism for the preparation of banana oil

why do you use sulfuric acid in the reaction

explain why we used simple distillation in order to isolate our product. Describe what is actually happening in the process.

Calculate and discuss your % yield...

explain why reflux is neccesary in this experiment..

When is it necessary to use a vacuum distillation? Give some explanation and provide examples

boiling point elevation of a solution containing 2.94 g sodium chloride and 114 g water

Question 1 Given the pair of reactions shown with the equilibrium constants, PCl3(g) + Cl2(g) ⇌ PCl5(g) K1 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) K2 What is the equilibrium constant for the reaction, PCl5(g + 2 NO(g) ⇌ PCl3(g) + 2 NOCl(g) A. K2/K1 B. K1/K2 C. K2‑K1 D. K1K2 .

Question 2 Given the reaction, 2 NO(g) + O2(g) ⇌ 2 NO2(g), for which the enthalpy of reaction is ‑118.9 kJ. Which one of the following will cause an increase in the equilibrium concentration of NO in a closed reaction chamber? A. adding some more O2(g) through an injection nozzle B. adding a catalyst C. increasing the pressure of the system while temperature is kept constant D. increasing the temperature of the system .

Question 3 Consider the following system, which is at equilibrium, 3 C(s) + 3 H2(g) ⇌ CH4(g) + C2H2(g) The result of removing some C(s) from the system will be: A. more C(s) is produced B. no further change occurs C. Kc increases D. more CH4(g) and C2H2(g) are produced to restore the equilibrium .

Question 4 A student is preparing a study of the reaction, 2 CO2(g) ⇌ 2 CO(g) + O2(g), for which Kc = 26.2 at 827 oC. What is the value of Kp at that same temperature? A. 3.86 x 10-1 B. 2.90 x 10-1 C. 2.36 x 10+3 D. 2.40 x 10+5

Can somone explain how you came up with the answers too. Thanks.

write structural formulas of each fragment and molecular ion on the ms spectrum of anise

Determine what is the temperature of the hot combustion gas that is produced in the engine of a butanol (C4H9OH)-burning bus that uses ambient air for the combustion. Tip: write the balanced stoichiometric equation for the combustion of butanol assuming air is composed of 80% N2 and 20% O2 by volume, and derive the energy balance of the combustion. Atomic weights: C-12, H-1, O-16, N-14. For butanol: cp = 2 kJ/kg/°C; cv = 1.75 kJ/kg/°C; heat released by combustion, or ΔH = 60 MJ/kg.

A fuel gas containing methane and ethane is burned with air in a furnace, producing a stack gas at 300.°C and 105 kPa (absolute). You analyze the stack gas and find that it contains no unburned hydrocarbons, oxygen, or carbon monoxide. You also determine the dew-point temperature.

(a) Estimate the range of possible dew-point temperatures by determining the dew points when the feed is either pure methane or pure ethane.

(b) Estimate the fraction of the feed that is methane if the measured dew-point temperature is 59.5°C

(c) What range of measured dew point temperatures would lead to calculated methane mole fractions within 5% of the value determined in Part (b).

describe steam distillation and it's advantages and limitations

abstract on how to isolate a spice essence and what techniques used to characterize it

The K_sp for M₂X₂, a slightly soluble ionic compound is 4.5 x 10^-29. The electron configuration of M₂⁺² is prepared Xe6s¹5d¹⁰4f¹⁴. The X^- anion has 54 electrons. What is the molar solubility of M₂X₂ in a solution of NaX prepared by dissolving 1.98 grams of NaX in water and diluting to 150 ml?

If you are given the following solids:

Na₃PO₄             MW = 163.94 g/mol

K₃PO₄                  MW = 212.26 g/mol   

NaH₂PO₄           MW = 119.98 g/mol

K₂HPO₄             MW = 174.17 g/mol

Na₂HPO₄           MW = 141.96 g/mol

KH₂PO₄             MW = 136.08 g/mol

Which compounds would you use to prepare your stock solutions? Why?

I picked KH2PO4 and K2HPO4 because potassium salts dissolve more readily in H2O which would make the lab go more smoothly. I would like to know if I'm missing any valuable pieces of information in this answer.

If you are given deionized water, the solid you selected in the previous question and the following volumetric glassware:

100.00 ml volumetric flask(s)

250.00 ml volumetric flask(s)

   25.00 ml volumetric transfer pipet(s)

   10.00 ml volumetric transfer pipet(s)

     5.00 ml volumetric transfer pipet(s)

            Describe how you would prepare the required stock solutions (two). Your explanation should be detailed and quantitative.  

what mass of Ca(NO₃)₂ must be added to 1.0 L of a 1.0 M HF solution to begin precipitation of CaF₂. You may assume no volume change on the addition of Ca(NO₃)₂. K_sp for CaF2 = 4.0 x 10^-11 and k_a for HF=7.2 x 10^-4.

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.) Part A 298 K