What is the name of CaCO3? Compounds in Science: Humans are constantly discovering new, innovative things. This is because those products are used for us to make life easier and more comfortable. In chemistry, the discovery of a compound like plastic has made carrying things lighter and durable.
How many grams of CaCO3CaCO3 are produced when 2.8 grams of CaOCaO reacts with excess CO2CO2?
The balanced reaction of calcium oxide and carbon dioxide to produce calcium carbonate shows the ratio by the number of moles of the three chemical species in the reaction. We can use the ratio to investigate the quantities in the reaction.
Answer to question 1
Answer and Explanation: CaCO3 is calcium carbonate, commonly known as limestone. It consists of calcium (Ca), carbon (C) and oxygen (O) elements. Calcium carbonate reacts to different processes. For example, the reaction of any acids with calcium carbonate releases carbon dioxide or when it combines with water and carbon dioxide to form calcium oxide. Calcium carbonate is found in the 4% of the earth’s crust. In fact, shells, eggs, pearls and marine organisms have the main component of calcium carbonate. It has a variety of uses like neutralizing pH in plants and acid rain, making cements, producing baking powder and relieving stomach gases using antacid.
Answer to question 2
Answer and Explanation:
The reaction above is balanced and, according to the reaction, the number of moles of CaO(s)CaO(s) used is the same as the number of moles of CaCO3CaCO3 produced.
For the calcium oxide, we have the following:
the mass of CaOCaO is m=2.8 gm=2.8 g.
the formula mass MM of CaOCaO equals the sum of the molar masses of 1 Ca atom and 1 O atom as in the formula, i.e., M=Ar(Ca)+Ar(O)=40.0 g/mole+16.0 g/mole=56.0 g/moleM=Ar(Ca)+Ar(O)=40.0 g/mole+16.0 g/mole=56.0 g/mole.
The number nn of moles of CaOCaO used equals the mass divided by the molar mass, i.e.:
n=mM=2.8 g56.0 g/mole=0.05 molesn=mM=2.8 g56.0 g/mole=0.05 moles
As established earlier, the number of moles of CaCO3CaCO3 produced is the same as the number of moles of CaOCaO used.
Here is what we have about the CaCO3CaCO3 in the reaction:
the number of moles of CaCO3CaCO3 is n=0.05 molesn=0.05 moles.
the molar mass of CaCO3CaCO3 equals the sum of the molar masses of the atoms 1 Ca, 1 c, and 3 O, i.e., M=Ar(Ca)+Ar(C)+3Ar(O)=40.0 g/mole+12.0 g/mole+3(16.0 g/mole)=100.0 g/moleM=Ar(Ca)+Ar(C)+3Ar(O)=40.0 g/mole+12.0 g/mole+3(16.0 g/mole)=100.0 g/mole.
The mass mm of CaCO3CaCO3 equals the product of the mass and the molar mass, i.e.:
m=nM=0.05 moles(100.0 g/mole)=5.0 gm=nM=0.05 moles(100.0 g/mole)=5.0 g
The mass of CaCO3CaCO3 produced is 5.0 g.
Answer to question 3
Since we know that given molecular reaction will be written as
CrSO4(aq) + Na2CO3(aq) = CrCO3(s) + Na2SO4(aq)
To write the net ionic equation storing electrolyte whic are in aqueous medium will dissociates into there ions .
Step 2 Ionic equation
Cr2+(aq) + SO42-(aq) + 2Na+(aq) + CO32-(aq) —–> CrSO3(s) + 2Na+ (aq) +SO42-(aq)
This is the Ionic equation .
Now , to write net ionic equation the spectator ions are cancelled out from both side .
Cr2+(aq) + CO32-(aq) —–> CrSO3(s)
This is the net Ionic equation.
Step 3 Answer
Cr2+(aq) + CO32-(aq) —–> CrSO3(s)
Answer to question 4
The names of the given compounds are as shown below.
Cu3N – Copper nitride
PbCl4 – Lead tetrachloride or lead (IV) chloride
CrSO3 – Chromium (II) sulfite