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4 years ago

5

Please help me! Thank you

2 answers:

elena55 [62]4 years ago

7 0

This reaction exothermic because the energy of the products (the straight line on the right side of the graph) is lower than the reactants (left the straight line).

an endothermic reaction will be the opposite.

Marta_Voda [28]4 years ago

5 0

The reaction is exothermic, the energy in the bonds has been released to the surroundings (causing the potential energy to go down). The increase in energy in the surrounding heats them up hence exothermic.

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Help me on this science question.

mel-nik [20]

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3 years ago

Sulfur dioxide has a vapor pressure of 462.7 mm Hg at –21.0 °C and a vapor pressure of 140.5 mm Hg at –44.0 °C. What is the enth

stealth61 [152]

Answer : The value of $\Delta H_{vap}$ is 28.97 kJ/mol

Explanation :

To calculate $\Delta H_{vap}$ of the reaction, we use clausius claypron equation, which is:

$\ln(\frac{P_2}{P_1})=\frac{\Delta H_{vap}}{R}[\frac{1}{T_1}-\frac{1}{T_2}]$

where,

$P_1$ = vapor pressure at temperature $-21.0^oC$ = 462.7 mmHg

$P_2$ = vapor pressure at temperature $-44.0^oC$ = 140.5 mmHg

$\Delta H_{vap}$ = Enthalpy of vaporization = ?

R = Gas constant = 8.314 J/mol K

$T_1$ = initial temperature = $-21.0^oC=[-21.0+273]K=252K$

$T_2$ = final temperature = $45^oC=[-41.0+273]K=232K$

Putting values in above equation, we get:

$\ln(\frac{140.5mmHg}{462.7mmHg})=\frac{\Delta H_{vap}}{8.314J/mol.K}[\frac{1}{252}-\frac{1}{232}]\\\\\Delta H_{vap}=28966.6J/mol=28.97kJ/mol$

Therefore, the value of $\Delta H_{vap}$ is 28.97 kJ/mol

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3 years ago

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3 years ago

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Spontaneous at low temperatures.

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2 years ago