A gas sample has a volume of 150 ml at 0.00 ∘c. the temperature is raised (at constant pressure) until the volume is 218 ml. wha
1 answer:
Charles law gives the relationship between volume and temperature of a gas.
It states that at constant pressure, volume is directly proportional to temperature of gas.
V/ T = k
where V -volume , T - temperature and k - constant
parameters for the first instance are given on the left side and parameters for the second instance are given on the right side of the equation
T1 - temperature in kelvin 0.0 °C + 273 = 273 K
substituting the values in the equation
T = 397 K
temperature in celcius - 397 K - 273 = 124 °C
new temperature is 124 °C
It states that at constant pressure, volume is directly proportional to temperature of gas.
V/ T = k
where V -volume , T - temperature and k - constant
parameters for the first instance are given on the left side and parameters for the second instance are given on the right side of the equation
T1 - temperature in kelvin 0.0 °C + 273 = 273 K
substituting the values in the equation
T = 397 K
temperature in celcius - 397 K - 273 = 124 °C
new temperature is 124 °C
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Answer:
A)
Explanation:
m = Mass of water = 38.9
M = Molar mass of water = 18 g/mol
= Avogadro's number =
The reaction of electrolysis would be
Number of moles of
From the reaction it can be seen that 2 moles of gives 1 mole of
So, number of moles of produced is
Number of molecules
So, of oxygen is produced.
The heat released in the combustion of lactic acid is absorbed by the
calorimeter and in the decomposition of the lactic acid.
ΔH°f of lactic acid is approximately <u>-716.2 kJ</u>
Reasons:
Known parameters are;
Mass of the lactic acid = 3.93 grams
Heat capacity of the bomb calorimeter = 10.80 kJ·K⁻¹
Change in temperature of the calorimeter, ΔT = 5.34 K
ΔHrxn = ΔErxn
ΔH°f of H₂O(l) = -285.8 kJ·mol⁻¹
ΔH°f of CO₂(g) = -393.5 kJ·mol⁻¹
The chemical equation for the reaction is presented as follows;
- C₃H₆O₃ + 2O₂ → 3CO₂ + 3H₂O
The heat of the reaction = 10.80 kJ·K⁻¹ × 5.34 K = 57.672 kJ
Molar mass of C₃H₆O₃ = 90.07 g/mol
Number of moles of C₃H₆O₃ = = 0.043633 moles
Number of moles of CO₂ produced = 3 × 0.043633 moles = 0.130899 moles
Heat produced = 0.130899 mole × -285.8 kJ·mol⁻¹ = -37.4109342 kJ
Moles of H₂O produced = 0.130899 moles
Heat produced = 0.130899 mole × -393.5 ≈ -51.51 kJ
Therefore, we have;
Heat absorbed by the lactic acid = ΔH°f of H₂O + ΔH°f of CO₂ + Heat absorbed by the calorimeter
Which gives;
Heat absorbed by lactic acid = -37.4109342 kJ - 51.51 kJ + 57.672 kJ ≈ -31.249 kJ
The heat absorbed by the lactic acid ≈ -31.249 kJ
ΔH°f of C₃H₆O₃ ≈ -716.2 kJ
Heat of formation of lactic acid ≈ <u>-716.2 kJ</u>.
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