Recent content by yang09

Thanks Borek. I got an answer to it

Forget what I said in the previous post about my work for Part B. I did not use the Ideal Gas law. What I did was that I used the percent weight of CO2 in the atmosphere and I set up the equation: 0.046 = (mass of CO2/mass of all gases in the atmosphere) X 100%. I assumed that the masses of all...

Thanks Borek for the help and explaining the things to me. It really cleared things up. I got the answer now for part A For Part B, I have a feeling that we will be using the ideal gas law again, except our pressure will be 1.0332 X 10^4 kg/ m2 instead of 1 atm and we will be solving for "n"...

Thanks for the help Borek and explaining step by step on how to go about solving the problem. I got an answer now. I appreciate it

So going back to the question, I know that one mole of carbon dioxide produces one mole of carbon. To clarify things up, in the ideal gas law, is the "n" we are solving for the moles of carbon dioxide since the question wants us to find the volume of air needed to support the 1 kg of Carbon. If...

What do you mean by an indirect assumption about the HCO3 - concentration? The way I solved for it was through the first dissociation step[ H2CO3--> HCO3- + H+]. I had an initial concentration of 0 for both HCO3- and H+ and solved the quadratic system for x, which was my HCO3- concentration.

Can you elaborate on what you mean here? What I did was that I did an I.C.E. Table ( I = initial concentration, C = Change in concentration, E = equation) and set up a quadratic equation with the 0.0023 M as the initial concentration of carbonic acid. Is that what you mean when you say...

The compound composition of CO2 are 2 atoms of Oxygen and 1 atom of Carbon. I am basing this off of the formula 1 mole of CO2 = 6.022 X 10^23 molecules of CO2 Since you have 1 atom of Carbon, you would also have 1 mole of carbon Am I right?

Sorry. My "x" value is of Carbonate, not dioxide. I mixed them up. Is my calculation of the minimum concentration of CO3 2- correct or atleast in the right ballpark? In order to solve for the [H] value from the second dissociation( HCO3 -<--> CO3 2- + H+), I would have use the first dissociation...

I assumed that the moles from glucose was the same as the moles of carbon because in the photosythesis process, CO2 is converted to carbon chains, which are then converted to glucose. I guess my thought process behind that was wrong then. To go from 1 mol of CO2 to molecules or atoms, I know...

So from the Photosynthesis formula, I know that 1 mol of Carbon(glucose) produces 6 moles of carbon dioxide. Here is my calculation: (1000g Carbon) X (1mol Carbon/12 g Carbon) X (6 mol CO2/1mol C) = 500 moles of CO2 (seems kind of big). My "n" that I used in the ideal gas law was the moles of...

To find the minimum concentration, what I did was I set up the Ksp of CaCO3: CaCO3 <--> [Ca2+][CO3 2-] and solved for CO3 2-. The Ksp of CaCO3 was 4.8 X 10^-9 so here was my setup: 4.8 X 10^-9 = [0.01][x]. I solved x, which is the concentration of Carbon Dioxide, to be 4.8 X 10^-7 M. From...

So x is the kg of Carbon dioxide. But we are not given a balanced equation to convert the 1kg of Carbon to kg of Carbon Dioxide. How would i go about and find the mass of Carbon Dioxide? I know that the 0.046% is the percent weight of Carbon Dioxide in the atmosphere so if I were to use the...

Homework Statement Shells of mussels are mainly of calcium carbonate. IUsually the shell is stable and its content is in equilibrium with the surrounding. Mussels need to build up or reduce their shell, however, for additional protection or during growth. They achieve this by changing the...

Im not really following your line of reasoning. Can you please explain further. From what I understand from your post is that our unknown is going to be the kg of Carbon Dioxide. Is that correct? Where do we go from there? What does IMHO stand for as well? Thanks