A mixture containing KCLO3, K2CO3, KHCO3, and KCL was heated, producing CO2, O2, and H2O (water) gases according following equations:

2KCLO3 -> 2KCL + O2
2KHCO3 -> K2O + H2O + 2CO2
2CO3 -> K2O + CO2

The KCL does not reacnder the conditions of the reaction. If 100.0g of the mixture produces 1.8g of H20, 13.2g of CO2, and 4g of O2, what was the compttion of the original mixture?(assume complete decomposition of the mixture)

someone please show me how to do this!
* all O'in the equations stand for oxygen, nothing means 20, its 2O, 2 then oxygen comes after.

O2 came from equation 1, so change the grams O2 to moles, then compute the moles and mass of potassium chlorate.

Water came only from equation 2, change the water mass to moles, and compute the moles/mass of potassium hydrogencarbonate. Also, compute the moles/mass of CO2 given off, subtract that from 13.2g. The remainder is given off in reaction 3. Repeat mole/mass relations to get the amount of K2CO3.
For the original amount of KCL, add the masses you found for KCLO3, KHCO3, and K2CO3, then subtract from 100g.

what is the name of the following compound K2O

To find the composition of the original mixture, we need to calculate the amount of each compound present based on the given products.

First, let's calculate the moles of H2O, CO2, and O2 produced:

Molar mass of H2O = 18 g/mol
Molar mass of CO2 = 44 g/mol
Molar mass of O2 = 32 g/mol

Moles of H2O = mass of H2O / molar mass of H2O = 1.8 g / 18 g/mol = 0.1 mol
Moles of CO2 = mass of CO2 / molar mass of CO2 = 13.2 g / 44 g/mol = 0.3 mol
Moles of O2 = mass of O2 / molar mass of O2 = 4 g / 32 g/mol = 0.125 mol

Now, let's determine the stoichiometry of the reactions to find the moles of each compound produced.

From the equation 2KHCO3 -> K2O + H2O + 2CO2, we can see that for every 2 moles of KHCO3, we produce 1 mole of H2O and 2 moles of CO2.

Moles of KHCO3 = 0.1 mol H2O × (2 mol KHCO3 / 1 mol H2O) = 0.2 mol KHCO3
Moles of CO2 from KHCO3 = 0.2 mol KHCO3 × (2 mol CO2 / 2 mol KHCO3) = 0.2 mol CO2

From the equation 2CO3 -> K2O + CO2, we can see that for every 1 mole of CO3 (which represents KCLO3, K2CO3, and KHCO3 combined), we produce 1 mole of CO2.

Moles of CO3 = 0.3 mol CO2
Moles of K2CO3 in original mixture = 0.3 mol CO3 × (1 mol K2CO3 / 1 mol CO3) = 0.3 mol K2CO3

We know that the mass of the mixture is 100 g, and we can use this information to find the remaining mass of KCL:

Mass of remaining compounds = mass of mixture - mass of H2O - mass of CO2 - mass of O2
Mass of remaining compounds = 100 g - 1.8 g - 13.2 g - 4 g = 81 g

Since the KCL does not react, the remaining 81 g must be composed of KCL, KCLO3, and KHCO3.

Moles of KCL = mass of KCL / molar mass of KCL
Moles of KCL = 81 g / (39.1 g/mol) = 2.07 mol KCL

Now, we need to calculate the moles of KCLO3 and KHCO3 based on the moles of KCL found.

From the equation 2KCLO3 -> 2KCL + O2, we can see that for every 2 moles of KCLO3, we produce 2 moles of KCL.

Moles of KCLO3 = moles of KCL = 2.07 mol

From the equation 2KHCO3 -> K2O + H2O + 2CO2, we can see that for every 2 moles of KHCO3, we produce 1 mole of H2O and 2 moles of CO2.

Moles of KHCO3 = moles of KCL / 2 = 2.07 mol / 2 = 1.04 mol

Now, let's summarize the composition of the original mixture:

- 2.07 mol of KCLO3
- 0.3 mol of K2CO3
- 1.04 mol of KHCO3
- 2.07 mol of KCL

Note that this answer assumes complete decomposition of the mixture as stated in the problem.

To find the composition of the original mixture, we need to determine the number of moles of each gas produced and use stoichiometry to calculate the amounts of individual components in the mixture. Here's the step-by-step solution:

1. Calculate the number of moles of H2O, CO2, and O2 produced:
- H2O: Given mass = 1.8g; molar mass of H2O = 18.015 g/mol
Moles of H2O = mass of H2O / molar mass of H2O = 1.8g / 18.015 g/mol
- CO2: Given mass = 13.2g; molar mass of CO2 = 44.01 g/mol
Moles of CO2 = mass of CO2 / molar mass of CO2 = 13.2g / 44.01 g/mol
- O2: Given mass = 4g; molar mass of O2 = 32.00 g/mol
Moles of O2 = mass of O2 / molar mass of O2 = 4g / 32.00 g/mol

2. Write down the balanced equations and determine the stoichiometric ratios:
- 2KHCO3 -> K2O + H2O + 2CO2 (From this equation, we can see that 2 moles of KHCO3 produce 1 mole of H2O and 2 moles of CO2)
- 2CO3 -> K2O + CO2 (From this equation, we can see that 2 moles of K2CO3 produce 1 mole of CO2)

3. Use the stoichiometric ratios to find the number of moles of KHCO3 and K2CO3 that contributed to the production of H2O and CO2:
- Moles of KHCO3 = 2 x Moles of H2O = 2 x (moles of H2O calculated in step 1)
- Moles of K2CO3 = 0.5 x Moles of CO2 = 0.5 x (moles of CO2 calculated in step 1)

4. Calculate the total number of moles of KHCO3, K2CO3, KCLO3, and KCL in the mixture:
- Moles of KCL = (moles of O2 calculated in step 1) / (moles of O2 produced per mole of KCLO3), which is 1 mole of O2 per mole of KCLO3 in the balanced equation.
- Moles of KCLO3 = Moles of KCL (since KCLO3 reacts to produce KCL)

5. Calculate the mass or percentage composition of each component in the mixture:
- Mass of KHCO3 = Moles of KHCO3 x Molar mass of KHCO3
- Mass of K2CO3 = Moles of K2CO3 x Molar mass of K2CO3
- Mass of KCLO3 = Moles of KCLO3 x Molar mass of KCLO3
- Mass of KCL = Moles of KCL x Molar mass of KCL

6. Convert the mass of each component to percentage composition:
- Percentage of KHCO3 = (Mass of KHCO3 / Total mass of the original mixture) x 100%
- Percentage of K2CO3 = (Mass of K2CO3 / Total mass of the original mixture) x 100%
- Percentage of KCLO3 = (Mass of KCLO3 / Total mass of the original mixture) x 100%
- Percentage of KCL = (Mass of KCL / Total mass of the original mixture) x 100%

Using these steps, you should be able to calculate the composition of the original mixture.