HF(g) + H2O(l) = H3O+(aq) + F-(aq)

In the following equilibrium in a closed system, indicate how the equilibrium is shifted by the indicated stress:

(a) Additional HF(g) is added to the system.
(b) Water is added.
(c) Ca(NO3)2 solution is added, and CaF2 precipitates. (d) The volume is reduced.
(e) KOH is added.
(f) A catalyst is added.

during the experiment, a student did not follow the procedure exactly as directed how will eact of these actions affect the weight of magnesium oxide( 7 on the report sheet)?

a-fumes were allowed to escape from the crucible(what is the compostion of the fumes)

b-water was not added to the crucible

c-the evaporation of water cused spattering

d-water was not completely removed by evaporation

2- the white powder often found on objects made of alminum is alminum oxide AL2O3 calculate the molar mass of the alminum oxide. if you wanted to make a molar quantity of alminum oxide in the lab how many Grams of alminum would you neeed to begin with?

3-a form of iron oxide commonrust has the formula Fe2O3 write a balanced equiation for its formation where would the oxygen come from?

4- if this experiment was carried out exactly as directed in the procudre section by a student in austrila for example should that student come up with a formula for the magnesium oxide other than MGO? why not ?

Calculate the enthalpy of the reaction

4B(s)+3O2(g)?2B2O3(s)

given the following pertinent information:

B2O3(s)+3H2O(g)?3O2(g)+B2H6(g),    ?H?A=+2035 kJ

2B(s)+3H2(g)?B2H6(g),                            ?H?B=+36 kJ

H2(g)+1/2O2(g)?H2O(l),                ?H?C=?285 kJ

H2O(l)?H2O(g),                                          ?H?D=+44 kJ

a sulfide of iron, containing 36.5% S by mass, is heated in O2(g), and the products are sulfur dioxide and an ioxide of iron containing 27.6% 0, by mass.

Write a balanced chemical question for this reaction.

Q: 50.00 ml of 0.5216 M copper(II) nitrate solution is combined with 100.0 ml of 0.5580 M potassium hydroxide solution according to the following unbalanced equation.

Cu(NO3)2 (ag) + KOH -> Cu(OH)2 (s) + KNO3 (aq)

(a) How many grams of copper(II) hydroxide can be formed?

(b) The solid was filtered, dried, and found to have a mass of 2.420 g. What was the percent yield?

(c) What are the concentrations of all species in the solution before the solid is removed?

Draw and label a schematic of an Ag/AgCl reference electrode. As part of your answer, include the ½ reaction that is utilized by this electrode and include a description of how reference electrodes are utilized in electrochemicalmeasurements

In radical chlorination of alkanes, non-equivalent hydrogens react with chlorine atoms at different rates. At 35

Give the expected ground-state electron configurations for the following elements:

a) Ti

b) Ru

c) Sn

d) Sr

e) Se

Please explain this process as well, thank you!

determine the [OH-] and pH of a solution tht is 0.140 M in F-.

9.Consider the exothermic equilibrium

2I(g) ? I₂(g)

What would be the effect on the position of equilibrium of

a.increasing the total pressure on the system by decreasing its volume. (2 points)

b.adding gaseous I₂ to the reaction mixture. (2 points)

c.decreasing the temperature. (2 points)

Please explain answers to get points, thanks!

A balloon is to be used to carry meteorological instruments to an elevation of 18000 feet. The balloon is filled with helium at the ground level temperature and pressure ( 70 degrees Fahrenheit, 1 atm). The balloon material weighs .001 lb per square foot. If the instruments weigh 12 lbs, what should the diameter be of the spherical balloon ? Assume the temperature to drop 10 degrees Fahrenheit for every 4000 feet height.

LiOH(s) + CO2(g) → Li2CO3(s) + H2O(l) If 92.4 grams of lithium hydroxide reacts with excess carbon dioxide, what mass of lithium carbonate will be produced?

Using the following data reactions:

How many moles of KMnO4 are equivalent to 1.000 mole of Fe2+?

In this exercise, weighed samples of a solid unknown containing NaCl and NaHCO₃react with hydrochloric acid. The volume of the CO₂ liberated by the reaction in the gas phase is measured with a gas collection syringe. From the volume we can calculate the number of moles of CO₂ in the gas phase using the ideal gas approximation.

Since the CO₂ is generated in an aqueous environment (aqueous HCl), some CO₂will dissolve in the liquid phase. The amount of CO₂ dissolved in the liquid phase is computed using Henry's Law which requires knowing the partial pressure of CO₂. As described in the exercise, this requires knowing the entire system gas volume in addition to the initial and final syringe readings.   

The entire system gas volume is the sum of the quantities labeled V_tube and V_syr in the diagram below, corrected for the liquid volume (the aqueous HCl).

The table below contains the data collected in one run of the reaction between an unknown and hydrochloric acid:

The following questions deal with the above data. The appropriate units are specified in the questions. Pay close attention to the number of significant figures in your answers.

1). What is the volume of CO₂ captured in the gas phase (in mL)?

2).What is the number of mmols of CO₂ captured in the gas phase? (Remember to account for the vapor pressure of water.)

3). What is the weight of the sample in grams?