Heat 1kg of CaCO3, get 560g of CaO.

Write the reactant equations and solve the mass of CO2 that born. The CaO is 100% pure.

Anyone help me, pls?

CaCO3 ==> CaO + CO2

mols CaCO3 = grams/molar mass = 1000/100 = about 10 mols.
Covert mols CaCO3 to mols CaO using the equations in the balanced equation. That is about 10 mols CaO since CaCO3:CaO is 1:1.
Convert mols CaO to grams. g = mols x molar mass = about 10 x 56 = about 560 so the yield is 100% which means the yield for CO2 will be 100%.
Now convert mols CaCO3 to mols CO2 and convert to grams as in the CaO to find grams CO2.

Sure, I would be happy to help! But first, I have a question for you. Did the CaCO3 turn into CaO completely or did it undergo partial decomposition?

To determine the mass of CO2 produced when heating 1kg of CaCO3, we first need to write the balanced chemical equation for the reaction. The reaction between CaCO3 and heat decomposes it into CaO and CO2.

The balanced equation for this reaction is:
CaCO3(s) -> CaO(s) + CO2(g)

According to the information provided, 1kg of CaCO3 is being heated, and it produces 560g of CaO. To find the mass of CO2 produced, we need to calculate the difference in mass between the initial mass of CaCO3 and the final mass of CaO.

Given:
Initial mass of CaCO3 = 1kg
Final mass of CaO = 560g

First, we convert the final mass of CaO to kg:
Final mass of CaO = 560g = 0.56kg

Now, we can calculate the mass of CO2 produced by subtracting the final mass of CaO from the initial mass of CaCO3:
Mass of CO2 = Initial mass of CaCO3 - Final mass of CaO
Mass of CO2 = 1kg - 0.56kg
Mass of CO2 = 0.44kg

Therefore, when heating 1kg of CaCO3, it produces 0.44kg (or 440g) of CO2.

Sure, I can help you with that!

To write the reactant equations and solve for the mass of CO2 produced when 1 kg of CaCO3 is heated to obtain 560 g of CaO, we need to understand the balanced chemical equation for the reaction between CaCO3 and heat.

The balanced chemical equation for the thermal decomposition of calcium carbonate (CaCO3) is as follows:
CaCO3(s) → CaO(s) + CO2(g)

From the equation, we can see that 1 mole of CaCO3 produces 1 mole of CaO and 1 mole of CO2.

To solve for the mass of CO2 produced, we can follow these steps:

Step 1: Calculate the number of moles of CaO produced.
The molar mass of CaO is 56.08 g/mol (40.08 g/mol for Ca + 16.00 g/mol for O). So, the number of moles of CaO produced can be calculated as:
moles of CaO = mass of CaO / molar mass of CaO
moles of CaO = 560 g / 56.08 g/mol
moles of CaO = 10 mol

Step 2: Since the balanced equation shows that the moles of CaO are equal to the moles of CO2, we can conclude that 10 moles of CO2 are produced.

Step 3: Calculate the mass of CO2 produced.
The molar mass of CO2 is 44.01 g/mol (12.01 g/mol for C + 2x16.00 g/mol for O). So, the mass of CO2 produced can be calculated as:
mass of CO2 = moles of CO2 x molar mass of CO2
mass of CO2 = 10 mol x 44.01 g/mol
mass of CO2 = 440.1 g

Therefore, when 1 kg of CaCO3 is heated to produce 560 g of CaO, approximately 440 g of CO2 is produced.

Note: The assumption made here is that all of the CaCO3 is converted to CaO without any losses or impurities.