Which of the following is the formation reaction for CaO(s)
Ca(s)+ 1/2O2(g)arrow Cao(s) is that right
Yes, with a modification or two. First, most profs won't allows fractions. To get rid of the fraction, just multiply everything through by 2.
2Ca + O2 ==> etc.
(You can place an arrow by using the equal sign as I have done plus a > sign OR a single line by using the hyphen-----> and the > sign.
Yes, you are correct. The formation reaction for CaO(s) can be represented by the equation:
Ca(s) + 1/2 O2(g) → CaO(s)
To determine if this equation correctly represents the formation reaction for CaO(s), we need to consider the following steps:
Step 1: Identify the reactants and products
In this equation, the reactants are Ca(s) (calcium metal) and O2(g) (oxygen gas), and the product is CaO(s) (calcium oxide solid).
Step 2: Balance the equation
To balance the equation, we need to make sure the number of atoms on both sides of the equation are equal. In this case, there is one calcium atom on both sides, so that is already balanced. However, there are two oxygen atoms on the left side (from O2) and only one oxygen atom on the right side (from CaO). To balance the oxygen atoms, we need to multiply CaO by 1/2:
Ca(s) + 1/2 O2(g) → CaO(s)
Step 3: Check if energy is required or released
In a formation reaction, energy is typically released. Since this equation does not indicate heat or any energy source, we can assume that the reaction releases energy (exothermic), which is typical for the formation of ionic compounds like CaO.
Therefore, the equation you provided, Ca(s) + 1/2 O2(g) → CaO(s), correctly represents the formation reaction for CaO(s).