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Alex_Xolod [135]
3 years ago
14

When 2 crystalline solid barium hydroxide octahydrate and crystalline solid ammonium nitrate are mixed in a beaker at room tempe

rature, a spontaneous reaction occurs. the temperature of the beaker contents rapidly falls to below 0º
c. use this information to decide whether the reaction is exothermic or endothermic and what the signs of δh and δs are?
Chemistry
1 answer:
podryga [215]3 years ago
5 0
It is endothermic reaction ΔH>0 (sign is +).
Because it is spontaneous reaction ΔG<span><0 (Gibbs free energy)
</span>ΔG=ΔH-TΔS, so must be TΔS>ΔH and ΔS<span>>0 (sign +).</span>
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If 10.0 mL of a .600 M of HNO3 reacts with 31.0 mL of .700M Ba(OH)2 solution, what is the molarity of Ba(OH)2 after the reaction
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Answer:

<u></u>

  • <u>0.456M</u>

Explanation:

<u>1. Balanced molecular equation</u>

     2HNO_3+Ba(OH)_2\rightarrow Ba(NO_3)_2+2H_2O

<u>2. Mole ratio</u>

     \dfrac{2molHNO_3}{1molBa(OH)_2}

<u>3. Moles of HNO₃</u>

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<u>4. Moles Ba(OH)₂</u>

  • n = 0.700M × 0.0310 liter = 0.0217 mol

<u>5. Limiting reactant</u>

Actual ratio:

   \dfrac{0.0600molHNO_3}{0.0217molBa(OH)_2}\approx0.28

Since the ratio of the moles of HNO₃ available to the moles of Ba(OH)₂ available is less than the theoretical mole ratio, HNO₃ is the limiting reactant.

Thus, 0.006 moles of HNO₃ will react completely with 0.003 moles of Ba(OH)₂ and 0.0217 - 0.003 = 0.0187 moles will be left over.

<u>6. Final molarity of Ba(OH)₂</u>

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