Chemistry Answers

Hello,

I've oxidated lead using electrolysis. I think it should be lead (iv) oxide ( I use 10 V power source and the color of the product is like color of Fe2O3). now I want to make lead (ii,iv) of it.

I've tryed heating it in a plate but it doesn't work. what should I do?

The first order rate of constant for the decomposition of a certain insecticide in water at 12degrees is 1.45/yr. A quantity of this is washed into the pond leading to a concentration of 5.0*10^-7M.calculate the halflife.

Human colour vision is “produced” by the nervous system based on how three different cone receptors interact with photons of light in the eye. These three different types of cones interact with photons of different frequency light, as indicated in the following chart:

Cone Type Range of Light Frequency Detected

S 6.00-7.49 x 1014 s-1

M 4.76-6.62 x 1014 s-1

L 4.28-6.00 x 1014 s-1

What wavelength ranges (and corresponding colours) do the three types of cones

detect?

How many grams are in 0.2 moles of beryllium iodide, BeI2?

2C2H6 + 7O2 = 4CO2 + 6H2O

1. How many moles of CO2 will be produced with 2 moles of C2H6?

2. How many moles of H2O will be produced with 14 moles of O2?

3. How many grams of H2O will be produced with 2 moles of C2H6?

4. How many grams of CO2 will be produced with 7 moles of O2?

5. If 105.68 grams of C2H6 reacts 89.35 grams O2

A. What is the limiting reagent?

B. What is the excess reagent?

C. How many grams of CO2 will be produced?

D. How many grams of H2O will be produced?

E. How many grams will be left from our excess reagent?

An oxide is a compound that contains at least one oxygen atom and only one other element in its chemical formula. Using your knowledge of chemistry comment on the chemistry of oxides.

Given the following thermochemical equations and the corresponding enthalpy change for each reaction, calculate the heat of combustion of acetylene gas, C2H2

1. 2C (graphite) + H2 (g)               C2H2(g)      ∆H= + 226.7 kJ
2. C(graphite) + O2 (g)             CO2(g)         ∆H= - 393.5 kJ
3.  H2(g) + ½ O2 (g)            H2O (l)                ∆H= - 285.8 kJ

0.30 mol C3H6O0.30 mol C3H6Othe amount of heat released during the combustion of:

1. 0.30 mol C3H6O
2. 100 g of C3H6O

Write the thermochemical equation for the following reactions that occur at constant pressure:

1. One mole ammonium nitrate dissolve in water to produce aqueous ammonium ion and nitrate ions, accompanied by the absorption of 28.1 kJ of heat
2. Formation of carbon dioxide gas from carbon (graphite) and oxygen, yields 393.5 kJ of heat

50.0 ml of 2.50M Sulfuric acid reacted with 43.5ml 2.75 Aluminum hydroxide. The reaction yielded Aluminum sulfate and water. (Al=27g/mol, S=32g/mol, H=1g/mol, O=16g/mol)

1. Write the balance chemical equation.

2. What is the limiting reactant?

3. How much reactant is in excess?

4. How many grams of Aluminum sulfate will be produced?