What do you understand by " hydrated ions" ? Give examples of hydrated ions and explain at least one hydrated ion's sturcture and formation.

1.) For the chemical reaction 2 Al + 3 H 2 SO 4 ⟶ 3 H 2 + Al 2 ( SO 4 ) 3 what mass of hydrogen is produced from 1.97 mol of aluminum?

2.) Convert 1.77×1024 atoms of carbon to moles of carbon.

1.77×1024 atoms=

3.)

Consider the combustion reaction for octane (C8H18), which is a primary component of gasoline.

2C8H18+25O2⟶16CO2+18H2O

How many moles of CO2 are emitted into the atmosphere when 17.1 g C8H18 is burned?

4.) For the reaction

2KI+Pb(NO3)2⟶PbI2+2KNO3how many grams of lead(II) iodide, PbI₂, are produced from 89.7 g of potassium iodide, KI?

5.)For the reaction

2NaOH+H2SO4⟶Na2SO4+2H2O

how many grams of sulfuric acid, H₂SO₄, are needed to react completely with 33.1 g of sodium hydroxide, NaOH?

PLEASE HELP...

Calculate the value of deltaG for the reaction

Si3N4 + 3O2 = 3 SiO2(alpha-quartz) + 2 N2

at 800 K. What percentage error occurs if it is assumed that deltaCp for the

reaction is zero?

The vapor pressure of chloroform (CHCl3) is 173 mm Hg at 25 °C. What is the vapor pressure of a solution consisting of 268 g of chloroform and 0.129 mol of a nonvolatile nonelectrolyte?

At the extreme limits (high and low end) of the plot of pH vs. log([HPO42-]/[H2PO4-]), the data points may appear as though they are leveling off. Think about the [HPO42-]/[H2PO4-] ratio at the extreme limits and explain why this leveling off occurs. (There is one other answer on Chegg but I do not understand the logic of that response) Thank you!

Research Question: How to determine the quantity of polyphenol oxidase in apple juice?

Over the course of the semester, we studied several techniques (spectrophotometry, acid-base titrations, redox experiments) to answer questions related to quantification and identification of compounds, kinetics of chemical reactions,and equilibrium constants. With some background research, write a researchable question that could be answered with one or more of the techniques used during the semester.Write a research plan to answer the question. The plan does not have to be a detailed step by step procedure, but an overview of the experiment including controls and how you would “work up” the data to answer your question.

A student ran the following reaction in the laboratory at 610 K:

CO(g) + Cl2(g) COCl2(g)

When she introduced 0.183 moles of CO(g) and 0.211 moles of Cl2(g) into a 1.00 liter container, she found the equilibrium concentration of Cl2(g) to be 6.72×10-2 M.  

Calculate the equilibrium constant, Kc, she obtained for this reaction.

2.A student ran the following reaction in the laboratory at 546 K:

COCl2(g) CO(g) + Cl2(g)  

When she introduced 0.854 moles of COCl2(g) into a 1.00 liter container, she found the equilibrium concentration of COCl2(g) to be 0.817 M.  

Calculate the equilibrium constant, Kc, she obtained for this reaction.

3. Consider the following reaction:

COCl2(g) CO(g) + Cl2(g)

If 6.56×10-3 moles of COCl2, 0.377 moles of CO, and 0.372 moles of Cl2 are at equilibrium in a 16.9 L container at 772 K, the value of the equilibrium constant, Kp, is

What is the pH of a buffer solution prepared by adding 15.0 g of ammonia chloide to 5.00 L of 0.200 M ammonia? Ka of ammonium is 5.8 x 10^-10

2) What is the pH of the buffer after 90.0mL of 2.00 M HCl are added?

3) What is the pH of the buffer if 15.00 g of NaOH is added to the original buffer solution?

40.00 mL of a 0.1000 M carbonic acid (H₂CO₃) was titrated with 0.2000 M sodium hydroxide.

carbonic acid pka1:6.35 pka2:10.33

1.Calculate the volume of sodium hydroxide required to reach the first equivalence point.

2.Calculate the volume of sodium hydroxide required to reach the second equivalence point.

3.Write the balanced acid-base reaction and calculate the pH before the addition of sodium hydroxide.

4.Write the balanced acid-base reaction and calculate the pH after the addition of 12.00 mL of sodium hydroxide

5.Write the balanced acid-base reaction and calculate the pH after the addition of 20.00 mL of sodium hydroxide

6. Write the balanced acid-base reaction and calculate the pH after the addition of 30.00 mL of sodium hydroxide

7.Write the balanced acid-base reaction and calculate the pH after the addition of 40.00 mL of sodium hydroxide

8.Write the balanced acid-base reaction (paper only) and calculate the pH after the addition of 44.00 mL of sodium hydroxide

to a 100.0 mL volumetric flask are added 1.00 mL volumes of three solutions: .0100 M AgNO3, .205 M NaBr, and .100 M NaCN. The mixture is diluted with deionized water to the mark and shaken vigerously. What mass of AgBr would precipitate from this mixture? Hint: The Ksp of AgBr is 5.4 x 10-13 and the Kf of Ag(CN)2- is 1.0 x 10^21

For the reaction shown below, the initial concentrations for reactants and products are as follows: [A] = 0.27 M, [B] = 0.0640 M, [C] = 0.0134 M, and [D] = 1.47 M. If the equilibrium constant for the reaction is K_C = 0.802, which direction does the reaction have to shift to reach equilibrium?

A + 3B ⇌ 2C + 3D

Enter 1 if it shifts left, 2 if it shifts right, or 3 if it's already at equilibrium.

A sample of carbonic acid (0.125 L, 0.199 M, pK_a1 = 6.35, pK_a2 = 10.33) was titrated with 1.75 M NaOH. Calculate the pH at the following points:

Before the titration.

At the 1st midpoint.

why are thermoset plastics not affected by solvents to the same extent as thermoplastics?

Phosphorus pentachloride is formed when phosphorus trichloride and chlorine react.

PCl_3(g) + Cl_2(g) ⇌ PCl_5(g)

The equilibrium constant for the reaction is K_C = 37.8 at 110 °C. If 0.887 mol of phosphorus trichloride is added to 0.550 mol of chlorine in a 1.02-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride?

Report your answer to THREE significant figures.

500 lbm/min hydrocarbon feed is pumped into the feed point halfway to the top of a distillation tower. The tower feed point is 40.0 feet above holding tank for the hydrocarbon. The pressure in the holding tank is 25.0 psia. The pressure in the tower at the feed point is 85.0 psia. Assume the energy lost due to friction is negligible. There is no significant change in velocity. The hydrocarbon density is 55.0 lbm/ft 3 . Calculate the pump power required in hp and watts.