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Since the question has pressure, temperature, and volume as variables, in order to arrive at an answer the combined gas law will be needed to arrive at an answer. The Combined Gas Law is a combination of Boyle's Law (pressure and volume are inversely proportional when temperature is constant) and Charle's Law (volume and temperature are proportional when pressure is constant) and is used when neither volume, pressure nor temperature is constant.
Combine Gas Law Equation: P₁V₁ ÷ T₁ = P₂V₂ ÷ T₂
The following values are what is known from the question:
the initial pressure (P₁) = 1 atm; the final pressure (P₂) is 0.5 atm,
the initial volume (V₁) = 300 mL or 0.3 L; the final volume (V₂) = 1 L
the initial temperature (T₁) = 27 °C
then we can substitute these into the equation to find the final temperature (T₂).
P₁V₁ ÷ T₁ = P₂V₂ ÷ T₂
∴ by substituting the known values,
⇒ (1 atm) (0.3 L ) ÷ (27 °C) = (0.5 atm)(1 L) ÷ T₂
⇒ T₂ = [ (0.5 atm) (1 L) (27 °C) ] ÷ (1 atm) (0.3 L )
⇒ T₂ = [13.5 atm · L · °C] ÷ [0.3 atm · L]
⇒ T₂ = 45 °C
Thus the new temperature of the gas is 45 °C.
Answer : The two spontaneous chemical reactions are:
Explanation :
Gibbs free energy : It is defined as the amount of energy that is available to do useful work.
A reaction to be spontaneous when
A reaction to be non-spontaneous when
For the reaction to be spontaneous, the Gibbs free energy of the reaction is negative or we can say that the value of is less than zero.
From the given chemical reactions we conclude that there are two reactions that are spontaneous (favorable).
The two spontaneous chemical reactions are:
Answer:
molar mass HA = 87.8 g/mole
Explanation:
Given 0.140g HA + 14.5ml(0.110M NaOH) => NaA + H₂O
Rxn is a 1:1 rxn ration => moles HA neutralized = moles NaOH used
=> 0.140g/molar mass of HA = (0.110M)(0.0145L)
=> molar mass of HA = (0.140g)/[(0.110moles/L)(0.0145L)] = 87.8 g/mole