In the following reaction, how many liters of carbon dioxide, CO2, measured at STP, would be produced from the decomposition of 143 g of magnesium carbonate, MgCO3?

MgCO3----MgO+CO2

for each mole of MgCO3, one gets one 22.4liters CO2.

143g of MgCO3 is how many moles?

answer is 38.0 L

To determine the volume of carbon dioxide (CO2) produced, we need to use the concept of stoichiometry and the given mass of magnesium carbonate (MgCO3).

1. Write the balanced chemical equation for the decomposition of magnesium carbonate:
MgCO3 → MgO + CO2

2. Calculate the molar mass of magnesium carbonate:
MgCO3 = (24.31 g/mol for Mg) + (12.01 g/mol for C) + (3 * 16.00 g/mol for O)
MgCO3 = 24.31 g/mol + 12.01 g/mol + 48.00 g/mol
MgCO3 = 84.32 g/mol

3. Convert the given mass of magnesium carbonate to moles:
moles of MgCO3 = mass / molar mass
moles of MgCO3 = 143 g / 84.32 g/mol
moles of MgCO3 ≈ 1.69 mol

4. Use the stoichiometric mole ratio between MgCO3 and CO2 to find the moles of CO2 produced:
From the balanced equation, we can see that one mole of MgCO3 produces one mole of CO2.
moles of CO2 = moles of MgCO3
moles of CO2 ≈ 1.69 mol

5. Apply the relationship between moles and volume of a gas at STP:
1 mole of any gas at STP occupies 22.4 liters of volume.

Therefore, the volume of carbon dioxide produced at STP is approximately equal to 1.69 moles × 22.4 liters/mole, which is approximately 37.9 liters.

To determine the number of liters of carbon dioxide (CO2) produced from the decomposition of magnesium carbonate (MgCO3), you will need to follow these steps:

Step 1: Balance the equation:
The balanced equation for the reaction is:
MgCO3 ---- MgO + CO2

Step 2: Calculate the molar mass:
The molar mass of MgCO3 is calculated by adding the atomic masses of each element in the compound. The atomic masses are:
Mg = 24.31 g/mol
C = 12.01 g/mol
O = 16.00 g/mol

Molar mass of MgCO3 = (1 * Mg) + (1 * C) + (3 * O) = 24.31 + 12.01 + (3 * 16.00) = 84.31 g/mol

Step 3: Convert grams to moles:
Use the given mass of magnesium carbonate (143 g) and the molar mass of MgCO3 (84.31 g/mol) to convert grams to moles.

Number of moles of MgCO3 = Mass of MgCO3 / Molar mass of MgCO3
= 143 g / 84.31 g/mol

Step 4: Determine the stoichiometry:
From the balanced equation, we can see that for every 1 mole of MgCO3 decomposed, 1 mole of CO2 is produced.

Since the number of moles of CO2 produced is equal to the number of moles of MgCO3 decomposed, the number of moles of CO2 is determined to be equal to 143 g / 84.31 g/mol.

Step 5: Convert moles to liters at STP:
At STP (Standard Temperature and Pressure), 1 mole of any ideal gas occupies 22.4 liters.

Number of liters of CO2 = Number of moles of CO2 * 22.4 liters/mol

By substituting the equation with the value found in step 4, we can calculate the number of liters of CO2 produced.

So, the final step is to multiply the number of moles of CO2 by 22.4 liters/mol to calculate the number of liters of CO2 produced.

Note: "STP" refers to standard temperature (0 degrees Celsius or 273.15 Kelvin) and standard pressure (1 atmosphere or 101.3 kilopascals).

I hope this explanation helps you understand the process of calculating the number of liters of CO2 produced from the given mass of magnesium carbonate.