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Inorganic Chemistry
Balance the following redox equations:
1. H2S + Cr2O72- → S + Cr3+ (acidic medium)
2. MnO2 + HCl → Mn2+ + Cl2 + H2O
1. H2S + Cr2O72- → S + Cr3+ (acidic medium)
2. MnO2 + HCl → Mn2+ + Cl2 + H2O
Inorganic Chemistry
Define the following:
1. Unimolecular reaction
2. Bimolecular reaction
3. Elementary reaction
4. Overall reaction
1. Unimolecular reaction
2. Bimolecular reaction
3. Elementary reaction
4. Overall reaction
Inorganic Chemistry
The equilibrium constant for the gaseous reaction
H2 + I2 ↔ 2HI is 50.2 at 448oC, calculate the number
of grams of HI that are in equilibrium with 1.25 mole of
H2 and 63.5g of Iodine at this temperature
H2 + I2 ↔ 2HI is 50.2 at 448oC, calculate the number
of grams of HI that are in equilibrium with 1.25 mole of
H2 and 63.5g of Iodine at this temperature
Inorganic Chemistry
if xyz=1, then prove that 1/xyz^-1+1/xzy^-1+1/yzx^-1 = 1
Inorganic Chemistry
Rubidium ignites spontaneously when exposed to oxygen to for rubidium
Rubidium ignites spontaneously when exposed to oxygen to for rubidium oxide. Rb²0. Rubidium exists as two isotopes (84.91u) and (86.91u). if the average atomic mass of rubidium is (84.91u), determine the percentage abundance of 85/37Rb
Rubidium ignites spontaneously when exposed to oxygen to for rubidium oxide. Rb²0. Rubidium exists as two isotopes (84.91u) and (86.91u). if the average atomic mass of rubidium is (84.91u), determine the percentage abundance of 85/37Rb
Inorganic Chemistry
why industrial usage of potassium hydroxide is 48% and if 100% is used, what is the effect of it?
Inorganic Chemistry
For the cell reaction represented as
Co/Co2+//Ni2+/Ni
Calculate the cell potential and free energy of reaction.
Co/Co2+//Ni2+/Ni
Calculate the cell potential and free energy of reaction.
Inorganic Chemistry
Write a balanced equation for each of the following nuclear reactions:
(A) uranium-230 undergoes alpha decay.
(B) bismuth-212 decays to polonium-212.
(A) uranium-230 undergoes alpha decay.
(B) bismuth-212 decays to polonium-212.
Inorganic Chemistry
What is the concentration of acetic acid and the pH in a solution that is 0.25% ionized?
Inorganic Chemistry
For the reaction between carbon and oxygen to form carbon monoxide, beginning with 0.85 mol of C,
2C(s) + O2(g) → 2CO(g)
how many moles of O2 are required to completely consume the C?
how many moles of CO are obtained when the C is completely reacted?
2C(s) + O2(g) → 2CO(g)
how many moles of O2 are required to completely consume the C?
how many moles of CO are obtained when the C is completely reacted?
