4 Carbon atoms in one molecule of Butane, times 2 because of two molecules, time the weight of one Carbon atom, which is 12 amu's (an amu = Atomic Mass unit, also known as a Dalton) equals 96 amu's.
2C4H10(g) + 13O2(g) ---> 8CO2(g) + 10H2O(g)Now, 96.3 grams(?) of carbon dioxide would be:m=96.3 n=m/MM=44.01 = (96.3)/(44.01)n=? = 2.19Now, the molar ration of butane:carbon dioxide1/4n(CO2) =n(C4H10)= .55 molfor butane:m=? m = nMM=58.24 = 31.86g butanen=.55
The molar mass of butane (C4H10) is 58.12 g/mol. The molar mass of hydrogen in butane is 10.81 g/mol. To calculate the mass percent of hydrogen in butane, you would divide the molar mass of hydrogen by the molar mass of butane and multiply by 100. This gives you a mass percent of approximately 18.6%.
The mass number for carbon is 12, which represents the total number of protons and neutrons in the nucleus of a carbon atom.
To calculate the percentage of carbon in C17H19NO3, first find the molar mass of the compound which is the sum of the molar masses of each element. The molar mass of C17H19NO3 is approximately 285.31 g/mol. Then calculate the molar mass contributed by carbon (17 carbon atoms) which is about 12.01 g/mol per carbon atom. The total mass contributed by carbon is 17 * 12.01 = 204.17 g/mol. Finally, express this mass as a percentage of the total molar mass: (204.17/285.31) * 100% ≈ 71.53%. So, carbon represents approximately 71.53% of the mass in C17H19NO3.
The physical property that is identical for butane and 2-methylpropane is their molecular formula, which is C4H10. Both compounds have the same number of carbon and hydrogen atoms per molecule.
2C4H10(g) + 13O2(g) ---> 8CO2(g) + 10H2O(g)Now, 96.3 grams(?) of carbon dioxide would be:m=96.3 n=m/MM=44.01 = (96.3)/(44.01)n=? = 2.19Now, the molar ration of butane:carbon dioxide1/4n(CO2) =n(C4H10)= .55 molfor butane:m=? m = nMM=58.24 = 31.86g butanen=.55
Matter is not created nor destroyed in chemical reactions, the total mass and number of atoms before the reaction equals the total number of atoms and mass after the reaction. Conservation of mass law.
The molar mass of butane (C4H10) is 58.12 g/mol. The molar mass of hydrogen in butane is 10.81 g/mol. To calculate the mass percent of hydrogen in butane, you would divide the molar mass of hydrogen by the molar mass of butane and multiply by 100. This gives you a mass percent of approximately 18.6%.
The molar mass of butane is 58,124; for mr explain this abbreviation.
The atomic mass of butane (C4H10) is approximately 58.12 grams/mol.
58
To determine the mass of carbon on the weighing dish, you would need to know the total mass of the dish plus the carbon. If, for example, the combined mass of the dish and carbon is 5.0 g, then the mass of the carbon alone would be 5.0 g - 1.0 g (mass of the dish) = 4.0 g. Without the total mass, the mass of carbon cannot be calculated.
Yes, air molecules do have mass. Air is made up of various gases such as nitrogen, oxygen, and carbon dioxide, and each of these gas molecules contributes to the overall mass of the air.
The atomic mass of carbon is approximately 12 atomic mass units. Therefore, the total mass of 100 carbon atoms would be 100 * 12 = 1200 atomic mass units.
The mass number for carbon is 12, which represents the total number of protons and neutrons in the nucleus of a carbon atom.
because of difference in structure propane (C3H8) has bigger molar mass then butane (C4H10) the molecules of butane are heavier and the forces between them are stronger as in propane, because of this more energy is needed to transfer liquid butane to gas
4.5*10^23