My teacher said this is a very hard question, but I'm trying to make an attempts. Can you guide me?
A biologist places a plant in a closed chamber. A sensor in the chamber maintains the carbon dioxide level at the normal atmospheric concentration of 0.03%. Another sensor allows the biologist to measure the amount of oxygen produced by the plant over time. If the plant produces 0.001 mole of oxygen in an hour, how much Carbon dioxide had to be added to the chamber during that hour to maintain the atmospheric concentration of 0.03%?
look at the balanced chemical reaction...
6CO2+ 6H2O >>6 O2 + C6H12O6
So for each mole of oxygen produced, one mole of carbon dioxide was used.
Thanks, but I'm still really confused (that seems to be my mantra lately). I haven't had chemistry for 2 years and I'm at a loss, where to next?
Help! I'm not sure where you got that equation from.
To solve this problem, you need to find the amount of carbon dioxide that needs to be added to the chamber in order to maintain a 0.03% concentration. Here's how you can approach the problem step by step:
Step 1: Understand the given information.
- The normal atmospheric concentration of carbon dioxide is 0.03%.
- The plant produces 0.001 mole of oxygen in an hour.
Step 2: Determine the molecular ratio between the production of oxygen and the consumption of carbon dioxide.
- To find the amount of carbon dioxide needed to produce a certain amount of oxygen, you can use the balanced equation for photosynthesis:
6CO2 + 6H2O → C6H12O6 + 6O2.
From this equation, you can see that for every mole of oxygen (O2) produced, 6 moles of carbon dioxide (CO2) are consumed.
Step 3: Calculate the amount of carbon dioxide needed.
- Divide the number of moles of oxygen produced (0.001 moles) by the stoichiometric coefficient of oxygen in the balanced equation (6 mol O2/mol CO2). This will give you the amount of carbon dioxide needed.
- 0.001 mol O2 / (6 mol CO2 / 1 mol O2) = 0.001/6 mol CO2 ≈ 0.00017 mol CO2.
Step 4: Calculate the volume or mass of carbon dioxide required.
- To find the volume or mass of carbon dioxide, you need to know the ideal gas law. The ideal gas law is given by PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature.
- However, in this problem, you are looking for the moles of carbon dioxide, and the question does not provide any additional information about pressure, volume, or temperature, so we cannot directly calculate the volume or mass of carbon dioxide.
Conclusion:
Based on the given information, you can determine that approximately 0.00017 moles of carbon dioxide needs to be added to the chamber in order to maintain the atmospheric concentration of 0.03%. However, without additional information, you cannot directly calculate the volume or mass of carbon dioxide needed.