1) Calcium carbonate comprises 40.0% calcium by weight.
M(CaCO₃)=100.1 g/mol
M(Ca)=40.1 g/mol
w(Ca)=40.1/100.1=0.400 (which is 40.0%)!
2) The mass fraction mentioned is superfluous information.
3) The resulting solution is:
m(Ca)=1.2 g
m(CaCO₃)=M(CaCO₃)*m(Ca)/M(Ca)
m(CaCO₃)=100.1g/mol*1.2g/40.1g/mol=3.0 g
1) The chemical equation is
Cu + 2AgNO3 ---> Cu (NO3)2 + 2Ag
2) Molar ratios are as follows:
1 mol Cu: 2 moles AgNO3: 1 mol Cu (NO3)2: 2 mol Ag
3) Converting 12.83 * 10^23 atoms of Cu to moles gives:
12.83 * 10^23 atoms / (6.02 * 10^23 atoms / mol) = 2.131 mol Cu
4) Using the ratios:
2.131 mol Cu * 2 mol Ag / 1 mol Cu = 4.262 mol Ag
5) To convert 4.262 mol of silver to grams, use the atomic weight of silver:
mass = moles × atomic mass = 4.262 mol * 107.9 g / mol = 459.9 grams
Answer: 459.9 g
The solution to your inquiry is: c = a + b - d. In the chemical equation aA + bB → cC + dD, c may take any value from 1 to however many are needed for the equation to maintain its balance. For instance, if we consider c + d = a + b, we can express c as a + b - d. If we assign values a = 1; b = 3, and d = 2, then c equals 1 + 3 - 2, resulting in c = 2, and so forth.
At standard temperature and pressure, it is established that 1 mole of gas has a volume of 22.4 liters.
According to the periodic table:
the molar mass of oxygen is 16 g
and the molar mass of hydrogen is 1 g
Hence, the molar mass of water vapor is calculated as 2(1) + 16 = 18 g
Thus, 18 g of water occupies 22.4 liters, therefore:
the volume for 32.7 g is (32.7 x 22.4) / 18 = 40.6933 liters
In a 100 g sample of the compound, there are 63.57 g of carbon, 6 g of hydrogen, 9.267 g of nitrogen, and 21.17 g of oxygen. First, convert these masses into moles (n) using the formula n = m/M, where M is the molar mass from the periodic table.
For carbon: 63.57 g C -> 63.57 g C / 12.01 g/mol = 5.29 moles C.
For hydrogen: 6 g H -> 6 g H / 1.008 g/mol = 5.95 moles H.
For nitrogen: 9.267 g N -> 9.267 g N / 14.01 g/mol = 0.6615 moles N.
For oxygen: 21.17 g O -> 21.17 g O / 16.00 g/mol = 1.32 moles O.
Thus, the mole ratio looks like this: C 5.29 H 5.95 N 0.6615 O 1.32.
Now, divide each value by the smallest number (1.32): C 4 H 4.5 N 0.5 O 1.
To eliminate fractions, multiply all values by 2, yielding C8H9N1O2.
Now, all numbers are integers! Hence, the empirical formula is C8H9NO2.
Although the empirical formula isn't always the same as the molecular formula, in this instance, it corresponds to acetaminophen.
