Inorganic Chemistry Answers

Electrochemical cells are constructed using different electrodes in Fe2+/Fe3+ (1M

electrolyte as shown in the figure below. Draw the Cyclic Voltammogram in a voltage range of 0-0.8V and describe the current contributions in cyclic voltammogram from each of the following electrodes:

. How many moles of O2 were needed for the combustion of the alcohol?

b. How many moles of H2O are formed for each mole of O2 consumed?

c. How many grammes of CO2 are produced for each mole of alcohol burned?

d. How many grammes of CO2 are produced for each gram of alcohol burned?

3. How many grams of ethanol, C6H12O is produced from 2000 grams of Glucose, C6H12O6?

how many grams p4 is formed for each mole of ca3(po4)2?

how many grammes of p4 is produced for each gram of ca3(po4)2 used?

how many moles sio2 is required for each mole of ca3(po4)2 used?

how many moles c is required for each mole of ca3(po4)2 used?

how many moles of p4 is formed for each mole of ca3(po4)2 used?

Write the dynamic model in eqn. 1 in terms of the deviation variables 0*(t), q*(t), and 0*(t)

Consider the following cell:

Ag | Ag+ (0.01M)||Ag+ (1M)|Ag

calculate the EMF of the cell at 298 K

The process of decomposition of an electrolyte by passing electric current through its solution is called as

How can you use a flame test to distinguish between hard and soft water

A 0.50 g sample of a Group 2 metal, M, was added to 40.0 cm3 of 1.00 mol dm–3 hydrochloric acid (an excess).

equation 1 M(s) + 2HCl (aq) → MCl 2(aq) + H2(g)

When the reaction had finished, the resulting solution was made up to 100 cm3 in a volumetric flask.

A 10.0 cm3 sample of the solution from the volumetric flask required 15.0 cm3 of 0.050 mol dm–3 sodium carbonate solution, Na2CO3, for complete neutralisation of the remaining hydrochloric acid.

Calculate the total amount, in moles, of hydrochloric acid remaining after the reaction shown in equation 1.

amount = ... mol

Use your answers to (a) and (b)(iv) to calculate the amount, in moles, of hydrochloric acid

that reacted with the 0.50 g sample of M.

amount = ... mol

Use your answer to (v) and equation 1 to calculate the amount, in moles, of M in the 0.50 g sample.

amount = ... mol Calculate the relative atomic mass, Ar, of M and identify M.

Ar of M = ... identity of M = ...

How can you use a flame test to distinguish between hard and soft water