0
Very close to 2. If it's all carbon-12, it will be exactly two, but there's enough carbon-13 in natural abundance carbon (about one part in a hundred) to bring the average Atomic Mass up to something like 12.011.
What else can I help you with?
How many carbon atom are in 5.60 g of glucose?
5.60 g C6H12O6 (1 mole C6H12O6/180.156 g)(6 moles C/1 mole C6H12O6)(6.022 X 1023/1 mole C) = 1.12 X 1023 atoms of carbon ======================
What statement about krypton is not true A its molar mass is 83.798 g per mol Kr B Its atomic number is 36 C one mole of krypton atoms has a mass of 41 point 90g D it is a noble gas?
Statement C is not true. One mole of krypton atoms has a mass of approximately 83.798 g, not 41.90 g.
What formulas give atom to atom mole to mole and atom to molecule ratios?
let's start with what a mole is... think of "a dozen".. what is that? 12 right? a dozen = 12 of anything.. 12 donuts. 12 people, 12 answers to this question.. agreed? A pair = 2 of anything...a pair of aces = 2 aces. Pair of shoes = 2 shoes. Pair of contact lenses = 2 lenses. etc.. pair = 2 a gross = 144 of anything.... right? bakers dozen = 13..... 13 cookies = a bakers dozen dozen, pair,gross and bakers dozen are all "labels" we give to a quantity of something.... right? a "mole" is just like dozen, pair, and gross etc. it is a label we give to a quantity of something. The number, though, is = 602,200,000,000,000,000,000,000... we usually write that as 6.022x10^23 a mole of donuts = 6.022x10^23 donuts a mole of answers = 6.022x10^23 answers. take awhile to read all those... a mole of people = 6.022x10^23 people... a mole of 1 dollar bills = $6.022x10^23 and just like 2 dozen donuts = 2 x 12 donuts = 24 donuts 2 moles of donuts = 2 x 6.022x10^23 donuts = 1.204x10^24 donuts got that down? Nothing mysterious. just a label. just like a dozen **************** now that you know what it is, how do we use it? First, we have a "mole" because the number of atoms of stuff that we can hold in our hand and see is HUGE. That is because atoms are tiny. In the lab, we would probably work with say a gram of something. probably about the size of a couple of aspirin. depending on the substance, that's probably about 1/10th of a mole = 6.022x10^22 atoms. so it's a convenient unit of measure. Rather than saying 60,220,000,000,000,000,000,000 atoms, we say 0.1 moles... ok? Next, the atomic masses listed on a periodic table are in units called "AMU's".. atomic mass units. and can be read as AMU per atom. but 1 amu = 1.66x10^-24 g and there are 6.022x10^23 atoms in 1 mole of atoms right? that's what a mole is now see if you can follow... (1 amu / atom) x (6.022x10^23 atoms / mole) x (1.66x10^-24 g / amu) = 1g / mole of atoms...usually just written g/mole notice what I've done? I've converted amu/atom to g/mole.. units of amu / amu cancel... atoms / atom cancel and we're left with g/mole What that gibberish means is this. You can read atomic mass on a periodic table as either amu/atom or g/mole... They are equivalent units. ********** Next. now that you have atomic mass in grams / mole what does that mean? for carbon 12, for example, atomic mass = 12.01 g / mole. that means if you have 12.01 g, you have 1 mole of Carbon 12. ie 6.022x10^23 atoms of carbon 12 if you have 3.01x10^23 atoms of carbon 12, you have 1/2 of a mole. since 1 mole weighs 12.01 g, you have 6.00 grams of Carbon.. See how that works? let's try a couple of practice problems a) calculate moles of C in 24.02 g C from the periodic table, the atomic mass of C = 12.01 amu/atom = 12.01 g/mole right? 24.02 g C x (1 mole C / 12.01 g C) = 2.000 moles C... g/g cancels.. b) calculate mass of C in 3.00 moles C 3.00 moles C x (12.01 g C / mole C) = 36.03 g C... moles / moles cancel c) calculate moles NaCl in 116.8 g NaCl... from periodic table mass Na = 23.0 g mass Cl = 35.4... so mass NaCl = 1x23 + 1x35.4 = 58.4 g/mole 116.8 g NaCl x (1 mole NaCl / 58.4 g) = 2.00 moles NaCl.. g/g cancels... leaves moles.. do you see that? d) how many atoms are in 2 moles of C? 2 moles x (6.022x10^23 atoms C / mole C) = 1.204x10^24 atoms NOTE: this takes practice. which is why you get assignments to do these conversions. Ok? practice. **************** when you start working in the lab and start working problems with chemical equations, moles are important. this is why... the coefficients of balanced chemical equations are mole ratios. not mass... 2 H2 + 1 O2 ---> 2 H2O... the 2,1,and 2 are MOLES (or you could read it as molecules also) 2 moles H2 reacts with 1 mole O2..ok? it ISN'T,2 grams of H2 reacts with 1 gram O2 to form 2 grams of H2O. so we convert masses to moles to use the balanced equations to calculate how much reactants we need and products we produce. whew... ask questions if you need to.. I'll check back in the morning. ****** as to the actual definition, a mole is technically defined as "the number of elemental entities in 12 g of carbon 12" = 6.022x10^23.
What is the mass of six helium atoms?
32 g
How do you get a chemistry mole?
One mole of something is 6.02 x 1023 (602,000,000,000,000,000,000,000) molicules (or atoms, if appropriate) of that substance. A gram molecular weight of anything will have one mole of molecules in it. Find out what substance you need a mole of, then find it's gram molecular weight. Take that much of the material (the gram molecular weight) and you've got your mole of that stuff.
How many Atoms are in 169g of c?
169 g C x 1 mole C/12.011 g x 6.02x10^23 atoms/mole = 8.47x10^24 atoms
How many atoms are in 24 grams of carbon?
28.5 g (6.02 x 1023 at / 12.01 g) = 1.43 x 1024atoms
How many atoms of carbon are in a pure sample of carbon having a mass of 72.0 g?
There are 6.022 x 10^23 atoms in 1 mole of carbon. The molar mass of carbon is 12 g/mol. Therefore, in 72.0 g of carbon, there are (72.0 g / 12 g/mol) * 6.022 x 10^23 atoms = 3.61 x 10^24 atoms of carbon.
How many carbon atoms are contained in 85.9 g of carbon?
85.9 (g C) = 85.9 (g C) / 12.00 (g/mol C) = 7.158 (mol C)7.158 (mol C)*[6.022*1023 (atoms/mol C)] = 4.31*1024 C-atoms
How many atoms are in a 12 g of C?
To find the number of carbon atoms in 12 g of carbon (C), you first need to calculate the number of moles of carbon (C) in 12 g using its molar mass. Then, you can use Avogadro's number (6.022 x 10^23) to determine the number of atoms in that many moles of carbon (C).
How many moles of C do you have in the CO2?
1 mole of CO2 has 1 mole of carbon atoms and 2 moles of oxygen atoms.
How many carbon atom are in 5.60 g of glucose?
5.60 g C6H12O6 (1 mole C6H12O6/180.156 g)(6 moles C/1 mole C6H12O6)(6.022 X 1023/1 mole C) = 1.12 X 1023 atoms of carbon ======================
What is the mass of atoms in grams of 1.02X10 to the 24 atoms Mn?
To find the mass of 1.02×10^24 atoms of Mn, you need to calculate the atomic mass of Mn from the periodic table (54.938045 g/mol). Then, divide the number of atoms by Avogadro's number to get moles, and finally multiply by the atomic mass to get the mass in grams. The mass of 1.02×10^24 atoms of Mn would be approximately 94.64 grams.
How many grams are in 1 mol nahco3?
1 mole of NaHCO3 Na = 1 * 22.99 g = 22.99 g H = 1 * 1.01 g = 1.01 g C = 1 * 12.01 g = 12.01 g O = 3 * 16.00 g = 48.00 g Total = 84.01 g There are 84.01 grams in one mole of NaHCO3.
What statement about krypton is not true A its molar mass is 83.798 g per mol Kr B Its atomic number is 36 C one mole of krypton atoms has a mass of 41 point 90g D it is a noble gas?
Statement C is not true. One mole of krypton atoms has a mass of approximately 83.798 g, not 41.90 g.
How many iron atoms are contained in 354 g of iron?
There are approximately 3.25 x 10^24 iron atoms in 354 g of iron. This calculation is done by converting the mass of iron to moles using the molar mass of iron, and then using Avogadro's number to convert moles to atoms.
What formulas give atom to atom mole to mole and atom to molecule ratios?
let's start with what a mole is... think of "a dozen".. what is that? 12 right? a dozen = 12 of anything.. 12 donuts. 12 people, 12 answers to this question.. agreed? A pair = 2 of anything...a pair of aces = 2 aces. Pair of shoes = 2 shoes. Pair of contact lenses = 2 lenses. etc.. pair = 2 a gross = 144 of anything.... right? bakers dozen = 13..... 13 cookies = a bakers dozen dozen, pair,gross and bakers dozen are all "labels" we give to a quantity of something.... right? a "mole" is just like dozen, pair, and gross etc. it is a label we give to a quantity of something. The number, though, is = 602,200,000,000,000,000,000,000... we usually write that as 6.022x10^23 a mole of donuts = 6.022x10^23 donuts a mole of answers = 6.022x10^23 answers. take awhile to read all those... a mole of people = 6.022x10^23 people... a mole of 1 dollar bills = $6.022x10^23 and just like 2 dozen donuts = 2 x 12 donuts = 24 donuts 2 moles of donuts = 2 x 6.022x10^23 donuts = 1.204x10^24 donuts got that down? Nothing mysterious. just a label. just like a dozen **************** now that you know what it is, how do we use it? First, we have a "mole" because the number of atoms of stuff that we can hold in our hand and see is HUGE. That is because atoms are tiny. In the lab, we would probably work with say a gram of something. probably about the size of a couple of aspirin. depending on the substance, that's probably about 1/10th of a mole = 6.022x10^22 atoms. so it's a convenient unit of measure. Rather than saying 60,220,000,000,000,000,000,000 atoms, we say 0.1 moles... ok? Next, the atomic masses listed on a periodic table are in units called "AMU's".. atomic mass units. and can be read as AMU per atom. but 1 amu = 1.66x10^-24 g and there are 6.022x10^23 atoms in 1 mole of atoms right? that's what a mole is now see if you can follow... (1 amu / atom) x (6.022x10^23 atoms / mole) x (1.66x10^-24 g / amu) = 1g / mole of atoms...usually just written g/mole notice what I've done? I've converted amu/atom to g/mole.. units of amu / amu cancel... atoms / atom cancel and we're left with g/mole What that gibberish means is this. You can read atomic mass on a periodic table as either amu/atom or g/mole... They are equivalent units. ********** Next. now that you have atomic mass in grams / mole what does that mean? for carbon 12, for example, atomic mass = 12.01 g / mole. that means if you have 12.01 g, you have 1 mole of Carbon 12. ie 6.022x10^23 atoms of carbon 12 if you have 3.01x10^23 atoms of carbon 12, you have 1/2 of a mole. since 1 mole weighs 12.01 g, you have 6.00 grams of Carbon.. See how that works? let's try a couple of practice problems a) calculate moles of C in 24.02 g C from the periodic table, the atomic mass of C = 12.01 amu/atom = 12.01 g/mole right? 24.02 g C x (1 mole C / 12.01 g C) = 2.000 moles C... g/g cancels.. b) calculate mass of C in 3.00 moles C 3.00 moles C x (12.01 g C / mole C) = 36.03 g C... moles / moles cancel c) calculate moles NaCl in 116.8 g NaCl... from periodic table mass Na = 23.0 g mass Cl = 35.4... so mass NaCl = 1x23 + 1x35.4 = 58.4 g/mole 116.8 g NaCl x (1 mole NaCl / 58.4 g) = 2.00 moles NaCl.. g/g cancels... leaves moles.. do you see that? d) how many atoms are in 2 moles of C? 2 moles x (6.022x10^23 atoms C / mole C) = 1.204x10^24 atoms NOTE: this takes practice. which is why you get assignments to do these conversions. Ok? practice. **************** when you start working in the lab and start working problems with chemical equations, moles are important. this is why... the coefficients of balanced chemical equations are mole ratios. not mass... 2 H2 + 1 O2 ---> 2 H2O... the 2,1,and 2 are MOLES (or you could read it as molecules also) 2 moles H2 reacts with 1 mole O2..ok? it ISN'T,2 grams of H2 reacts with 1 gram O2 to form 2 grams of H2O. so we convert masses to moles to use the balanced equations to calculate how much reactants we need and products we produce. whew... ask questions if you need to.. I'll check back in the morning. ****** as to the actual definition, a mole is technically defined as "the number of elemental entities in 12 g of carbon 12" = 6.022x10^23.
