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kirill [66]
2 years ago
6

If the reaction 2HgO --> 2Hg + O2 is endothermic, which bonds are the strongest?

Chemistry
1 answer:
Alika [10]2 years ago
3 0
  • Endothermic reaction means the reactant side takes heat from surrounding and get decomposed i.e ∆H=-ve
  • If the equation is exothermic then it means the reactant is happy to decompose .But it's not as it's endothermic

Now

  • HgO is Omitted from our solution option.

Hg is a atom so no bonds hence no bond strength occurs.

  • O_2 is a molecule and so it's our answer .
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Given the unbalanced reaction: P₄+ O₂ <img src="https://tex.z-dn.net/?f=%5Crightarrow" id="TexFormula1" title="\rightarrow" alt=
alex41 [277]

Answer:

The correct answer is option e.

Explanation:

P_4+ 5O_2 \rightarrow P_4O_{10}

Moles of phosphorus pent-oxide :

\frac{14.2 g}{284 g/mol}=0.05 mol

According to reaction, 1 mole of phosphorus pent-oxide is obtained from 5 moles of oxygen gas.

Then 0.05 mole of  phosphorus pent-oxide will be obtained from:

\frac{5}{1}\times 0.05 mol=0.25 mol

Hence,the correct answer is option e.

6 0
3 years ago
Given the following, determine ΔG°f at 298 K for SnO. Sn(s) + SnO2(s) → 2SnO(s) ; ΔG° = 12.0 kJ at 298K
Virty [35]

Answer:

The value of change in Gibbs free energy for tin(II) oxide solid is -251.9 kJ/mol.

Explanation:

Sn(s) + SnO_2(s)\rightarrow 2SnO(s), \Delta G_{f}^{o} = 12.0 kJ

\Delta G_{f,SnO_2}^{o}= -515.8kJ/mol

\Delta G_{f,Sn}^{o}= 0 kJ/mol

\Delta G_{f,SnO}^{o}=?

\Delta G_{f}^{o}=\sum ((\Delta G_{f}^{o})_ {products})-\sum ((\Delta G_{f}^{o})_ {reactants})

12.0 kJ=(2 mol\times \Delta G_{f,SnO}^{o})-(1mol\times 0 kJ/mol+1 mol\times -515.8 kJ/mol)

\Delta G_{f,SnO}^{o}=-251.9 kJ/mol

The value of change in Gibbs free energy for tin(II) oxide solid is -251.9 kJ/mol.

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