How many grams of KCl would be formed in the reaction of 3.000 g of K2CO3 and HCl?

write and balance the equation.

then figure the moles of potassium carbonate.

Look at the mole ratio of KCl to potassium carbonate.

Multipy the originalmoles of postassium carbonate by that ratio, and you have the moles of KCl. Convert that to grams.

To determine the number of grams of KCl formed in the reaction between K2CO3 and HCl, we need to use the concept of stoichiometry. The balanced equation for the reaction is:

2K2CO3 + 2HCl -> 4KCl + CO2 + H2O

From the balanced equation, we can see that 2 moles of K2CO3 react with 2 moles of HCl to produce 4 moles of KCl. We can use this information along with the molar masses of the compounds to calculate the grams of KCl formed.

Step 1: Calculate the molar mass of K2CO3

The molar mass of each element in K2CO3 is:
2 potassium (K) atoms = 2 * 39.10 g/mol = 78.20 g/mol
1 carbon (C) atom = 12.01 g/mol
3 oxygen (O) atoms = 3 * 16.00 g/mol = 48.00 g/mol

Adding up the molar masses: 78.20 + 12.01 + 48.00 = 138.21 g/mol

Step 2: Calculate the number of moles of K2CO3

Using the given mass of K2CO3 (3.000 g) and the molar mass of K2CO3 (138.21 g/mol), we can calculate the number of moles of K2CO3 using the formula:

moles = mass / molar mass

moles of K2CO3 = 3.000 g / 138.21 g/mol

Step 3: Calculate the number of moles of KCl

Since the reaction is balanced in a 1:4 ratio of K2CO3 to KCl, the number of moles of KCl formed is the same as the number of moles of K2CO3:

moles of KCl = moles of K2CO3

Step 4: Calculate the mass of KCl

To find the mass of KCl, multiply the number of moles of KCl by its molar mass.
The molar mass of KCl is the sum of the molar masses of potassium (K) and chlorine (Cl):

molar mass of KCl = 39.10 + 35.45 = 74.55 g/mol

mass of KCl = moles of KCl * molar mass of KCl

Substitute the moles of KCl (from step 3) into the equation to get the mass of KCl.

mass of KCl = moles of KCl * 74.55 g/mol

Now, you can solve for the number of grams of KCl formed in the reaction using the calculated moles of KCl and the molar mass of KCl.