Inorganic Chemistry Answers

the metabolism of glucose in a living cells provides energy for their functioning. how many grams of oxygen are used in the metabolism of 1.009 glucose?

Dear Sir/Madam

can you please answer this question for me.

thanks in advance

​1-Chloropropane was hydrolysed by an aqueous potassium hydroxide solution. 

   C3H7Cl   +  KOH   →    C3H7OH    +   KCl  

​​   1-Chloropropane​           Propan-1-ol

​During the reaction, the reactant potassium hydroxide is used up. Samples of the reaction mixture were drawn off at regular time intervals and analysed by titration with standard hydrochloric acid to find out the concentration of KOH. 

    The results are given in the table below:

Time / s

Concentration of OH-  / mol dm-3

0.500

100

0.350

200

0.250

300

0.180

400

0.125

500

0.090

600

0.063

       700

0.040

800

0.030

​​​​​

(a)

From the above information, Plot a Concentration of OH- (mol dm-3) against Time (s) graph. The graph MUST be a hand drawn (plotted) graph. 

(b)

Select 4 suitable points along your graph [see part (a)] and draw tangents to find the rates. Construct a table of “Rate” against “Concentration”. Note: The rates need to be calculated and the calculations shown.

(c)

Plot a graph of Rate against Concentration of OH-. The graph MUST be a hand drawn (plotted) graph.

(d)

From your graph in part (c) deduce the Order of Reactionwith respect to OH- (hydroxide ions).

(

(e)

Write a rate equation with respect to concentration of hydroxide ions.

(f)

Calculate the rate constant k from the gradient of the graph, drawn in part (c). Show and explain your working.

Answer the following stoichiometry questions by referring to the equation below:

2  KClO₃  →  2 KCl + 3 O₂

i.      If 1.50 mol of KClO₃ decomposes, what is the mass of O₂ that will be produced?

ii.     If 80.0 grams of O₂ was produced, how many moles of KClO₃ are decomposed?

iii.    Find the mass of KClO₃ needed if we need to produce 2.75  mol of KCl.

The chromatograms in the picture below show the separation of a two-component mixture. The Liquid

Chromatography column is 25 cm long. The flow rate was 0.40 ml/min. Using the chromatograph to

answer the following questions.

Source: Test Bank Hage/Carr Analytical Chemistry & Quantitative Analysis C. McLaughlin

1. Determine the dead time of the chromatographic analysis

(1 marks)

2. Determine the retention time of compounds A and B

(2 Marks)

3. Calculated the adjusted retention time of the compound A and B

(2 marks)

4. Calculated the capacity factor (k’) for compounds A and B

(4 marks)

5. Calculate the selectivity factor between peaks A and B

(2 marks)

6. Discuss the influence of reducing the flowrate on selectivity factor

(5 Marks)

7. Discuss the separation between compound A and B as shown on the chromatograph

(3 Marks)

8. Calculate the number of theoretical plates involved in the separation of A and B

Dear Sir/Madam

can you please answer this question for me.

thanks in advance

​1-Chloropropane was hydrolysed by an aqueous potassium hydroxide solution. 

   C3H7Cl   +  KOH   →    C3H7OH    +   KCl  

​​   1-Chloropropane​           Propan-1-ol

​During the reaction, the reactant potassium hydroxide is used up. Samples of the reaction mixture were drawn off at regular time intervals and analysed by titration with standard hydrochloric acid to find out the concentration of KOH. 

    The results are given in the table below:

Time / s

Concentration of OH-  / mol dm-3

0.500

100

0.350

200

0.250

300

0.180

400

0.125

500

0.090

600

0.063

       700

0.040

800

0.030

​​​​​

(a)

From the above information, Plot a Concentration of OH- (mol dm-3) against Time (s) graph. The graph MUST be a hand drawn (plotted) graph. 

(b)

Select 4 suitable points along your graph [see part (a)] and draw tangents to find the rates. Construct a table of “Rate” against “Concentration”. Note: The rates need to be calculated and the calculations shown.

(c)

Plot a graph of Rate against Concentration of OH-. The graph MUST be a hand drawn (plotted) graph.

(d)

From your graph in part (c) deduce the Order of Reactionwith respect to OH- (hydroxide ions).

(

(e)

Write a rate equation with respect to concentration of hydroxide ions.

(f)

Calculate the rate constant k from the gradient of the graph, drawn in part (c). Show and explain your working.

Reaction between lead(ii) nitrate and sodium iodide to produce lead(ii) iodide and sodium nitrate

Procedure:Use electron dot structures to predict the formulas of the ionic compounds formed from the following elements:

  1) 200.0 g of Ca(C2H3O2)2 was found in the chemistry laboratory.  

    Calculate 

a) . the volume at STP if Ca(C2H3O2)2 is converted to gas.     

b) .  the molarity of a solution made by dissolving 200.0 g of Ca(C2H3O2)2 in 200 mls of water

A) A 1.00 g gaseous sample of hydrocarbon occupies a volume of 385 mL at 330 K and 1.00 atm. Find the molar mass of the compound.

B) Calculate the number of atoms of He(g) that are needed to exert a pressure of 4.0 X 10–2 kPa in a 15 mL container at a temperature of –23°C.

95.0 grams of I₂O₅, reacts with 45.0 grams of carbon monoxide, CO, in the reaction described below. If the percentage yield is 93.0% calculate the actual yield of CO₂ in grams.