Inorganic Chemistry Answers

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

      Calculate

          i. the molecular mass of 1 mole Ca(C₂H₃O₂) _2.

         ii. the number of  moles of Ca(C₂H₃O₂)₂  that exists   

        iii. the number of Ca(C₂H₃O₂)₂ molecules present

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

        v.  the molarity of a solution made by dissolving 200.0 g of      

                Ca(C₂H₃O₂)₂ in 200 ml of water

Calculate the number of atoms of He(g) that are needed to exert a pressure of 4.0 atm in a 15 mL container at a temperature of -23℃

a metal has a specific heat capacity of .899 Jg-1k-1 How much energy is required to raise the temperature of 2.00 Kg of the metal by 80 K

5g of calcium carbonate was strongly heated to a constant mass calculate the mas of the solid residue formed Ca=40.0,O=16.0,C=12

Discuss the position of copper family in periodic table

1. When baking soda was mixed with vinegar, effervescence was observed.

What caused the effervescence?

2. How can you conclude that the reaction has gone to completion?

3. Which balloon has the least amount of air inside?

4. Which balloon has the most air inside?

5. Will the balloon size grow bigger if more vinegar is in the bottle? Why?

6. Will it take more time to complete the reaction if there were more vinegar in the bottle with the

same amount of baking soda?

7. Which is the limiting reagent?

8. Which is the reagent in excess?​

What are degrees of freedom? What is the maximum number of degrees of freedom possible for a one-component system?

` 4.Define any five of the following terms : (i) A component (ii) Critical point (iii) molar conductivity (iv) Transference number (v) Standard hydrogen electrode (vi) Electrolytic cells`

A compound has mass percentage of 65.450%carbon and 5.492%Hydrogen and 29.060%Oxygen. It has a molar mass of approximately 110grams per mol. Determine the molecular formula of the compound

Steel wool , which is made of pure iron metal, burns with oxygen gas to produce ferric oxide (Fe2O3). Fe(s) + O2(g) ( Fe2O3

If there are 1.25 moles of Fe and 1.25 moles of O2,

How many moles of Fe2O3 will be produced? What is its mass?

If the actual laboratory yield is 95.8g Fe2O3, what is the rection’s percent yield?

Pure aluminum (Al) metal reacts with hydrocholoric acid (HCl) to produce aluminum chloride (AlCl3) and hydrogen (H2) gas.

Write the balanced chemical equation for the reaction described above.

If the expected mass of AlCl3 to be formed is 3.5g, what should be the initial mass of the pure aluminum metal?

If the actual mass of AlCl3 produced is 3.1g, what is the percentage yield of the reaction?