Answer:
CO2 < CH3Br < CH3OH < RbF
Explanation:
The boiling point of the compounds can be determined in terms of the strength of the intermolecular forces present in each compound.
Intermolecular forces are weak forces joining non-polar and polar molecules together. We have London dispersion forces, dipole-dipole forces of attraction, and hydrogen bonding.
London dispersion forces are weak attractions found between non-polar and polar symmetrical molecules. They are the weakest of all the electrical forces and they act between atoms and molecules e.g CO2
The dipole-dipole attractions are forces of attraction existing between polar unsymmetrical molecules. The dipole-dipole force of attractions is much stronger than London dispersion forces but weaker than Hydrogen bonding. e.g CH3Br
Hydrogen bonding is a special dipole-dipole attraction between polar molecules in which a hydrogen atom is directly joined to a highly electronegative atom (e.g. oxygen, nitrogen, or fluorine). Here, the bond in CH3OH is a hydrogen bond.
Ionic bonding is a bond that is formed between two kinds of atoms having a large electronegative difference such as in RbF,
Thus, in increasing order of boiling point;
CO2 < CH3Br < CH3OH < RbF
First, we will use the general gas formula to get the number of moles.
PV = nRT where:
P is the pressure of gas = 751 mmHg = 100125.096375 Pascal
V is the volume = 1 liter = 0.001 m^3
n is the number of moles we want to calculate
R is the gas constant = <span>8.314 J/(K. </span>mol<span>)
T is the temperature = 31 degrees celcius = </span>304.15 degree kelvin
Substitute in the above equation to get the number of moles as follows:
100125.096375 * 0.001 = n * 8.314 * 304.15
n = 0.039595 moles
Now, we will use the number of moles to get the mass as follows:
number of moles = mass / molar mass
mass = number of moles * molar mass
number of moles = 0.039595 moles
molar mass of ammonia (NH3) = 14 + 3(1) = 17 grams
Substitute to get the mass as follows:
mass = 0.039595 * 17 = 0.673122 grams
Last step is to get the density as follows:
density = mass / volume
mass = 0.673122 grams
volume = 1 liter
density = 0.673122 / 1 = 0.673122 grams/liter = <span>0.000675 kg/L</span>
Answer:
The common oxide of nitrogen that has a positive ΔS°f is nitric oxide (NO)
Explanation:
Without reference to thermodynamic data, we have;
1) N₂ (g) + O₂ (g) ⇄ 2 NO (g)
1 unit of N₂ + 1 unit of O₂ (total of 2 units) gives 2 units of NO, (Increase of +0 disorder)
∴ΔS°f = +ve
2) 2NO + O₂ → 2NO₂
2 unit of NO + 1 unit of O₂ (total of 3 units) gives 2 units of NO₂, (Decrease of disorder)
∴ΔS°f = -ve
3) N₂ + 1/2 O₂ → N₂O
1 unit of N₂ + 1/2 unit of O₂ (total of 1+1/2 units) gives 2 units of NO₂, (Decrease of disorder)
∴ΔS°f = -ve
4) 4 NO₂ + O₂ → 2N₂O₅
4 unit of NO₂ + 1 unit of O₂ (total of 5 units) gives 2 units of N₂O₅, (Decrease of disorder)
∴ΔS°f = -ve
5) NO + NO₂ ⇄ N₂O₃
1 unit of NO + 1 unit of NO₂ (total of 2 units) gives 1 unit of N₂O₃, (Decrease of disorder)
∴ΔS°f = -ve
Therefore, the common oxide of nitrogen that has a positive ΔS°f without reference to thermodynamic data is nitric oxide NO.
Main function of haemoglobin in the body is to transport oxygen to every cell/organ of the body
Hope this helps!!
<u>Given information:</u>
Mass of H2 = 2 g
Mass of O2 = 32 g
<u>To determine:</u>
Mass of H2O2 produced
<u>Explanation:</u>
The reaction between H2 and O2 can be given as:
H2 + O2 → H2O2
Based on the reaction stoichiometry:
1 mole of H2 reacts with 1 mole of O2 to form 1 mole of H2O2
# moles of H2 = mass of H2 / molar mass of H2 = 2 g/ 2 g.mol-1 = 1 mole
# moles of O2 = mass of O2/ molar mass of O2 = 32 g/ 32 g.mol-1 = 1 mole
Hence for the given reactant conditions, moles of H2O2 produced = 1
Mass of H2O2 = moles of H2O2 * molar mass H2O2 = 1 mole * 34 g.mole-1 = 34 g
<u>Ans</u>: 34 g of H2O2 is produced in this reaction
