when 2.76 (0.0200 mol) of k2co3 was mixed with 30.0 ml of approximately 2 M HCL the temperature rose by 5.2 C
how do i write a balanced equation for problems like this?
K2CO3+ HCl (aq)>>CO2+K2O+H2O> KOH +CO2
Note the second reaction is with K2O with the water that accompanies the acid. 2M HCl is mostly water.
To write a balanced equation for a chemical reaction, you need to identify the reactants and products involved. In this case, we have K2CO3 (potassium carbonate) and HCl (hydrochloric acid) reacting to form products. The reactants are K2CO3 and HCl, and the products are formed as a result of their chemical reaction.
Here's how you can write the balanced equation for this reaction:
1. Start by writing the formula equation using the chemical formulas of the reactants and products:
K2CO3 + HCl → products
2. Next, balance the equation by ensuring that the number of atoms on each side of the equation is the same. Begin by balancing the complex molecules or polyatomic ions first, followed by the individual elements.
Let's balance the equation step by step:
a) Balance the potassium (K) atoms:
On the left side, we have 2 potassium (K) atoms in the K2CO3 molecule. To balance this, we assign a coefficient '2' to the HCl molecule:
K2CO3 + 2HCl → products
b) Balance the chlorine (Cl) atoms:
On the right side, we have 2 chlorine (Cl) atoms in 2HCl molecule. To balance this, we assign a coefficient '2' to the KCl product:
K2CO3 + 2HCl → 2KCl + products
c) Balance the carbon (C) and oxygen (O) atoms:
On the left side, we have 1 carbon (C) and 3 oxygen (O) atoms in the K2CO3 molecule. To balance this, we assign a coefficient '1' to the CO2 product:
K2CO3 + 2HCl → 2KCl + CO2 + products
Now you have the balanced equation:
K2CO3 + 2HCl → 2KCl + CO2 + products
This equation represents the chemical reaction between potassium carbonate (K2CO3) and hydrochloric acid (HCl) in which potassium chloride (KCl) and carbon dioxide (CO2) are produced. The "products" part of the equation will depend on the specific reaction conditions and other factors that were not provided in the given information.