With radiocarbon dating, scientists compare an object's carbon-14 levels with _____. the carbon-14 levels of an object from the
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Q1)
we can use the ideal gas law equation to find the total pressure of the system ;
PV = nRT
where P - pressure
V - volume - 7 x 10⁻³ m³
n - number of moles
total number of moles - 0.477 + 0.265 + 0.115 = 0.857 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature in K - 273 + 25 °C = 298 K
substituting the values in the equation
P x 7 x 10⁻³ m³ = 0.857 mol x 8.314 Jmol⁻¹K⁻¹ x 298 K
P = 303.33 kPa
1 atm = 101.325 kPa
Therefore total pressure - 303.33 kPa / 101.325 kPa/atm = 2.99 atm
Q2)
partial pressure is the pressure exerted by the individual gases in the mixture.
partial pressure for each gas can be calculated by multiplying the total pressure by mole fraction of the individual gas.
total number of moles - 0.477 + 0.265 + 0.115 = 0.857 mol
mole fraction of He -
mole fraction of Ne -
mole fraction of Ar -
partial pressure - total pressure x mole fraction
partial pressure of He - 2.99 atm x 0.557 = 1.67 atm
partial pressure of Ne - 2.99 atm x 0.309 = 0.924 atm
partial pressure of Ar - 2.99 atm x 0.134 = 0.401 atm
we can use the ideal gas law equation to find the total pressure of the system ;
PV = nRT
where P - pressure
V - volume - 7 x 10⁻³ m³
n - number of moles
total number of moles - 0.477 + 0.265 + 0.115 = 0.857 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature in K - 273 + 25 °C = 298 K
substituting the values in the equation
P x 7 x 10⁻³ m³ = 0.857 mol x 8.314 Jmol⁻¹K⁻¹ x 298 K
P = 303.33 kPa
1 atm = 101.325 kPa
Therefore total pressure - 303.33 kPa / 101.325 kPa/atm = 2.99 atm
Q2)
partial pressure is the pressure exerted by the individual gases in the mixture.
partial pressure for each gas can be calculated by multiplying the total pressure by mole fraction of the individual gas.
total number of moles - 0.477 + 0.265 + 0.115 = 0.857 mol
mole fraction of He -
mole fraction of Ne -
mole fraction of Ar -
partial pressure - total pressure x mole fraction
partial pressure of He - 2.99 atm x 0.557 = 1.67 atm
partial pressure of Ne - 2.99 atm x 0.309 = 0.924 atm
partial pressure of Ar - 2.99 atm x 0.134 = 0.401 atm
Explanation:
Entropy is defined as the degree of randomness present in a substance. Therefore, more is the irregularity present in a compound more will be its molar entropy.
Hence, decreasing order to molar entropy in state of matter is as follows.
Gases > Liquids > Solids
- In the first pair, we are given
or
. Since, molar entropy of liquids is less than the molar entropy of gases.
Hence, will have larger molar entropy as compared to
.
- In the second pair, we are given Fe(s) or Ni(s). More is the molar mass of a compound more will its molar entropy. Molar mass of Fe is 55.84 g/mol and molar mass of Ni is 58.69 g/mol.
Hence, molar entropy of Ni(s) is more than the molar entropy of Fe(s).
- In the third pair, we are given
or
. As both the given species are gaseous in nature. So, more is the molar mass of specie more will be its molar entropy.
Molar mass of is 30.07 g/mol and molar mass of
is 28.05 g/mol. Therefore, molar entropy of
is more than the molar entropy of
.
- In the fourth pair, we are given
or
. Molar mass of
Therefore, molar entropy of is more than the molar entropy of
.
- In the fifth pair, we are given HgO(s) or MgO(s). Molar mass of HgO is 216.59 g/mol and molar mass of MgO is 40.30 g/mol.
Hence, molar entropy of HgO(s) is more than the molar entropy of MgO.
- In the fifth pair, we are given NaCl(aq) or
. Molar mass of NaCl 58.44 g/mol and molar mass of
Hence, the molar entropy of is more than the molar entropy of NaCl(aq).