The intial temperature : 59.865 °C
<h3>Further explanation</h3>
Heat added :
Q = m . c . ΔT
Q = heat, J
m = mass, g
c = specific heat, joules / g ° C
∆T = temperature difference, ° C / K
Answer : Carbon tetrachloride, will show the greatest freezing point lowering.
Explanation :
For non-electrolyte solution, the formula used for lowering in freezing point is,
where,
= lowering in freezing point
= molal depression constant
m = molality
As per question, the molality is same for all the non-electrolyte solution. So, the lowering in freezing point is depend on the only.
That means the higher the value of , the higher will be the freezing point lowering.
From the given non-electrolyte solutions, the value of of carbon tetrachloride is higher than the other solutions.
Therefore, Carbon tetrachloride, will show the greatest freezing point lowering.
<u>Answer:</u> The standard Gibbs free energy of the reaction is -15.8 kJ/mol
<u>Explanation:</u>
Relation between standard Gibbs free energy and equilibrium constant follows:
where,
= Standard Gibbs free energy = ?
R = Gas constant =
T = temperature = 298 K
= equilibrium constant = 581
Putting values in above equation, we get:
Conversion factor used: 1 kJ = 1000 J
Hence, the standard Gibbs free energy of the reaction is -15.8 kJ/mol
Its empirical formula : C₅H₁₂O₆
<h3>Further explanation </h3>
The empirical formula is the smallest comparison of atoms of compound forming elements.
<em>(empirical formula) n = molecular formula </em>
The principle of determining empirical formula and molecular formula
- Determine the mass ratio of the constituent elements of the compound.
- Determine the mole ratio by dividing the elemental mass with the relative atomic mass obtained by the empirical formula
Ar C = 12 g/mol
Ar H = 1 g/mol
Ar O = 16 g/mol
mol ratio of C : H : O =
Number of moles= Mass/Molar Mass= 200g/(12,011 g/mol)=16,651 Moles
Molar Mass of Carbon = 12,011 g/mol