2LiOH + CO2 yields Li2CO3 + H2O will the astronauts survive and how much water is made if there is 2.00 kg LiOh and expel 35kg of CO2?
Here is a worked example of a stoichiometry problem.
Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
To determine if the astronauts will survive and how much water is produced, we need to calculate the amount of reactants consumed and products formed based on the given values. Let's break it down step by step:
1. Write down the balanced chemical equation:
2 LiOH + CO2 -> Li2CO3 + H2O
2. Calculate the molar masses:
- Molar mass of LiOH = atomic mass of Li (6.941 g/mol) + atomic mass of O (15.999 g/mol) + atomic mass of H (1.008 g/mol) = 23.95 g/mol
- Molar mass of CO2 = atomic mass of C (12.01 g/mol) + 2 * atomic mass of O = 12.01 g/mol + 2 * 15.999 g/mol = 44.01 g/mol
3. Convert the given masses of LiOH and CO2 to moles:
- Moles of LiOH = mass of LiOH / molar mass of LiOH = 2000 g / 23.95 g/mol = 83.42 mol
- Moles of CO2 = mass of CO2 / molar mass of CO2 = 35000 g / 44.01 g/mol = 793.42 mol
4. Determine the limiting reactant:
In the balanced equation, the stoichiometric ratio between LiOH and CO2 is 2:1. Therefore, 2 moles of LiOH react with 1 mole of CO2. To determine the limiting reactant, we need to compare the moles of LiOH and CO2. Since we have 83.42 mol of LiOH and 793.42 mol of CO2, CO2 is the limiting reactant because you need twice the amount of LiOH to react with the given amount of CO2.
5. Calculate the moles of products:
Since CO2 is the limiting reactant, it will completely react, forming the same number of moles of Li2CO3 and water. Therefore,
- Moles of Li2CO3 = 793.42 mol
- Moles of H2O = 793.42 mol
6. Calculate the mass of water formed:
- Mass of water = moles of H2O * molar mass of H2O = 793.42 mol * (2 * 1.008 g/mol + 15.999 g/mol) = 25321.48 g = 25.32 kg
Now, to answer your questions:
Will the astronauts survive?
Based on the reaction, the astronauts will survive as there is no indication of any harm caused by the reaction.
How much water is made?
From the given reactant masses, 25.32 kg of water will be formed.
Keep in mind that this calculation assumes ideal conditions and complete conversion of reactants to products. In reality, some factors such as incomplete reactions or other side reactions may affect the actual outcome.