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barxatty [35]
3 years ago
15

Why doesnt iron burst into flames when it rusts

Chemistry
1 answer:
Katarina [22]3 years ago
3 0
Rust does not have the properties to catch onto flames. However, if you light it on fire, then it would probably catch in flames but not instantly and will not continue to burn unless you have soaked it in oil or flammable object or substance. :) Hope this helps! 
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Consider the malate dehydrogenase reaction from the citric acid cycle. Given the listed concentrations, calculate the free energ
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<u>Answer:</u> The Gibbs free energy of the reaction is 21.32 kJ/mol

<u>Explanation:</u>

The chemical equation follows:

\text{Malate }+NAD^+\rightleftharpoons \text{Oxaloacetate }+NADH

The equation used to Gibbs free energy of the reaction follows:

\Delta G=\Delta G^o+RT\ln K_{eq}

where,

\Delta G = free energy of the reaction

\Delta G^o = standard Gibbs free energy = 29.7 kJ/mol = 29700 J/mol  (Conversion factor: 1 kJ = 1000 J)

R = Gas constant = 8.314J/K mol

T = Temperature = 37^oC=[273+37]K=310K

K_{eq} = Ratio of concentration of products and reactants = \frac{\text{[Oxaloacetate]}[NADH]}{\text{[Malate]}[NAD^+]}

\text{[Oxaloacetate]}=0.130mM

[NADH]=2.0\times 10^2mM

\text{[Malate]}=1.37mM

[NAD^+]=490mM

Putting values in above expression, we get:

\Delta G=29700J/mol+(8.314J/K.mol\times 310K\times \ln (\frac{0.130\times 2.0\times 10^2}{1.37\times 490}))\\\\\Delta G=21320.7J/mol=21.32kJ/mol

Hence, the Gibbs free energy of the reaction is 21.32 kJ/mol

4 0
3 years ago
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