well, in one molecule of CO2 there is 1 carbon atom and 2 oxygen atom, similarly, in 10 CO2, there will be 10 C atoms and 20 Oxygen atom and extending this forwards, in one mole of CO2, there will be one mole of Carbon atom and 2 moles of O atom. Remember, mole is just a number. and it is equal to 6.022 * 10^23 particles.
But CH3 isn't really stable, is it? Wouldn't the H:C ratio imply a formula of CxH3x, rather than simply CH3? The most straightforward formula that fits and is of a real hydrocarbon is C2H6, it seems to me. What am I missing?
@@9-volt247 I mean, I'm still here as in "watching TH-cam on a regular basis." I'm not really lurking in the comments section of this video at this point, since that was three years ago. Why do you ask? Do you have more to add to this thread?
I don't understand how having 0.128 moles of CO2 is the same as having 0.128 moles of C, and that having 0.1927 moles of H20, H2 just 0.1927 * 2? My logic is that the moles of C02 would be larger than just O (because CO2 is comprised of 2 elements rather than just one). And the moles of H20 would be a larger number than just H2 (because H20 is comprised of two elements rather than just one). Help!
In one molecule of CO2, you have 1 C atom and 2 O atoms. So, in 2 molecules of CO2, you have 2 C and 4 O. Thus in 1 mole of CO2, you have 1 mole of C and 2 moles of O. Keep in mind that a mole is just a quantity.
It makes sense when i think about it but moles are kinda funky and go against my instincts so i think it would be best to avoid converting to moles until the end to avoid making mistakes, the concept of the mole just beckons them.
How 1mol of c / 1 mol of co2? Really a doubt
well, in one molecule of CO2 there is 1 carbon atom and 2 oxygen atom, similarly, in 10 CO2, there will be 10 C atoms and 20 Oxygen atom and extending this forwards, in one mole of CO2, there will be one mole of Carbon atom and 2 moles of O atom. Remember, mole is just a number. and it is equal to 6.022 * 10^23 particles.
That orange dot is really in the way....
But CH3 isn't really stable, is it? Wouldn't the H:C ratio imply a formula of CxH3x, rather than simply CH3? The most straightforward formula that fits and is of a real hydrocarbon is C2H6, it seems to me. What am I missing?
u are missing the fact that its the empirical formula and not the molecular formula
@@praiseprince_ Just looked up "empirical formula" versus "molecular formula", and that clears things up. Thanks!
@@9-volt247 I mean, I'm still here as in "watching TH-cam on a regular basis." I'm not really lurking in the comments section of this video at this point, since that was three years ago. Why do you ask? Do you have more to add to this thread?
I don't understand how having 0.128 moles of CO2 is the same as having 0.128 moles of C, and that having 0.1927 moles of H20, H2 just 0.1927 * 2?
My logic is that the moles of C02 would be larger than just O (because CO2 is comprised of 2 elements rather than just one). And the moles of H20 would be a larger number than just H2 (because H20 is comprised of two elements rather than just one).
Help!
In one molecule of CO2, you have 1 C atom and 2 O atoms. So, in 2 molecules of CO2, you have 2 C and 4 O. Thus in 1 mole of CO2, you have 1 mole of C and 2 moles of O. Keep in mind that a mole is just a quantity.
it do be like that big man
1 mol of CO2 has 1 mol of C
So 0.128 CO2 will have 0.128 mol of C
It makes sense when i think about it but moles are kinda funky and go against my instincts so i think it would be best to avoid converting to moles until the end to avoid making mistakes, the concept of the mole just beckons them.