A. Potassium oxide
B. Calcium chloride
C. Magnesium nitride
D. Sodium hypochlorite
E. Potassium nitrate
Pan 4: theyre the smallest and most broken down :)
Heat the sulfuric acid solution and adding copper carbonate in it.
<h3>Improvement require in this experiment</h3>
The method could be improved by heating sulfuric acid solution and add copper carbonate into the solution of sulfuric acid. Add the copper carbonate until it is present in excess amount. After that filter the extra amount of copper carbonate so in this way the blue copper sulfate crystals are produced.
Learn more about copper here: brainly.com/question/3157958
Answer:
The particles must be in the correct orientation upon impact.
The particles must collide with enough energy to meet the activation energy of the reaction.
Explanation:
This a problem related to chemical kinetics. The collision theory is one of the theories of reaction rates and it perfectly explains how the effectiveness of colliding molecules dictates the pace of a reaction.
For reactions to occur, there must be collisions between reacting particles. It implies that the collision per unit time and how successful collisions are determines the rate of chemical reactions in most cases. Therefore, for a collision to be successful, colliding particle must have enough energy which is greater than the activation energy of the reaction. In order to also produce the desired products, the colliding particles must be properly oriented.
Now ,
C + O2 → CO2
According to above equation, 1 mole of carbon reacts with one mole of oxygen to produce one mole of carbon dioxide.Thus this implies that 12 g of carbon reacts with 32 g of O2 to produce 44 g of CO2.
No of moles = mass of the substance/molecular mass of the substance.
In this case 1.2 g of carbon reacts with "x "g of O2 to produce 4.4 g of CO2.
No of moles of carbon in this case = 1.2÷ 12 = 0.1 moles.
No of moles of carbon dioxide formed = 4.4÷44 =0.1 moles
Thus already discussed above, 1 mole of carbon reacts with 1 mole of oxygen to produce 1 mole of carbon dioxide. Hence to produce 0.1 mole of CO2 ,0.1 mole of carbon needs to react with 0.1 mole of oxygen.
Also number of moles of O2 = mass of O2÷ molar mass of O2
Substituting number of moles of O2 as 0.1 we get
mass of O2(x) = Number of moles of O2 × Molar mass of O2
Mass of O2 (x) = 0.1 × 32= 3.2 g
Thus mass of 3.2 g O2 reacts with 1.2 g of CO2 to produce 4.4 g of CO2.
