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daser333 [38]
3 years ago
5

Put an x of it is a physical property but of it is a chemical propety pit a +

Chemistry
1 answer:
makkiz [27]3 years ago
4 0
  • Density=a+
  • Flammability=a
  • Solubility=a
  • Reacts with acid to form H2=a+
  • Support combustion=a+
  • Sour taste=a
  • Melting point=a
  • Boiling point=a
  • Hardness=a
  • luster=a+
  • Odor=a
  • Maleability =a
  • Shiny=a
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The chemical equilibrium will shift to the left.
Since NH4+ ions are a product of the original reaction, increasing their concentration will shift the equilibrium toward the reactants.
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What’s the Difference between attractive forces and ionic/covalent/metallic bonds
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Given that ΔH = −571.6 kJ/mol for the reaction 2 H2(g) + O2(g) → 2 H2O(l), calculate ΔH for these reactions. (a) 2 H2O(l) → 2 H2
pashok25 [27]

Answer : The value of \Delta H for the reaction is +571.6 kJ/mole.

Explanation :

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction is,

2H_2(g)+O_2(g)\rightarrow 2H_2O(l)     \Delta H_1=-571.6kJ/mole

Now we have to determine the value of \Delta H for the following reaction i.e,

2H_2O(l)\rightarrow 2H_2(g)+O_2(g)    \Delta H_2=?

According to the Hess’s law, if we reverse the reaction then the sign of \Delta H change.

So, the value \Delta H_2 for the reaction will be:

\Delta H_2=-(-571.6kJ/mole)

\Delta H_2=+571.6kJ/mole

Hence, the value of \Delta H for the reaction is +571.6 kJ/mole.

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