When surface water dissolves carbon dioxide, carbonic acid (H2CO3) is formed. When the water moves underground through limestone formations, the limestone dissolves and caves are sometimes produced.
CaCO3(s) + H2CO3(aq) Ca(HCO3)2(aq)
What mass of limestone must have dissolved if 4.93 1010 kg of calcium hydrogen carbonate was produced?
would the correct answer be 3.04e13??
i found this by taking 4.93e10kg converting it to grams= 4.93e13g Ca(HCO3)2 then converting that to moles and then setting that equal to limestone (CacCO3) and converting that then to grams.
Yes, I obtained 3.04 x 10^10 kg and that is 3.04 x 10^13 g CaCO3.
yes that is the right answer, thanks Dr.bob
Well, well, well, looks like we have a chemistry question here! Let's see if we can solve it with a touch of humor.
To find out the mass of limestone that dissolved, we need to follow the steps you mentioned. So, buckle up and enjoy the ride!
First, we convert 4.93 × 10^10 kg to grams. That's a lot of grams! It's a good thing we don't have to count them all out individually. Phew!
Next, we convert this mass to moles of calcium hydrogen carbonate (Ca(HCO3)2). I don't know about you, but I imagine moles wearing tiny lab coats and tiny goggles. Just picture that for a second!
Now that we have moles of Ca(HCO3)2, it's time to set up a mole-to-mole conversion with limestone (CaCO3). We like conversions in this process, don't we? It's like a chemistry-themed carnival!
Finally, we convert moles of limestone to grams to get our final answer. And drum roll, please...
The correct answer is... 3.04 × 10^13 grams! You got it right!
Congratulations on solving the problem, my friend! You deserve a chemistry-themed party with lots of balloons and test tube-shaped confetti. Keep up the great work!
To find the mass of limestone that must have dissolved, we can use stoichiometry and the given balanced equation:
CaCO3(s) + H2CO3(aq) → Ca(HCO3)2(aq)
We are given the mass (4.93 × 10^10 kg) of calcium hydrogen carbonate (Ca(HCO3)2) produced and we need to find the mass of limestone (CaCO3) that dissolved.
Here are the step-by-step calculations:
1. Convert the mass of calcium hydrogen carbonate produced to grams:
4.93 × 10^10 kg × 1000 g/kg = 4.93 × 10^13 g
2. Calculate the molar mass of calcium hydrogen carbonate (Ca(HCO3)2):
Ca(HCO3)2 = 1(Ca) + 2(H) + 2(C) + 6(O) = 40.08 + 2.02 + 24.02 + 96.00 = 162.12 g/mol
3. Convert the mass of calcium hydrogen carbonate produced to moles:
Moles of Ca(HCO3)2 = Mass(g) / Molar mass(g/mol)
Moles of Ca(HCO3)2 = (4.93 × 10^13 g) / (162.12 g/mol) = 3.04 × 10^11 mol
4. From the balanced equation, we can see that one mole of calcium hydrogen carbonate is formed from one mole of limestone (CaCO3).
5. Convert the moles of calcium hydrogen carbonate to moles of limestone:
Moles of CaCO3 = Moles of Ca(HCO3)2
6. Calculate the molar mass of limestone (CaCO3):
CaCO3 = 1(Ca) + 1(C) + 3(O) = 40.08 + 12.01 + 48.00 = 100.09 g/mol
7. Convert the moles of limestone to grams:
Mass of CaCO3 = Moles of CaCO3 × Molar mass(g/mol)
Mass of CaCO3 = (3.04 × 10^11 mol) × (100.09 g/mol) = 3.04 × 10^13 g
Therefore, the correct answer is 3.04 × 10^13 grams, confirming your result.