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ArbitrLikvidat [17]
2 years ago
12

When the reaction 2H₂S(g) ↔️2H₂(g) + S2(g) is carried out at 1065°C, Kp = 0.012. Starting with pure H₂S at 1065°C, what must the

initial pressure of H₂S be if the equilibrated mixture at this temperature is to contain 0.250 atm of H₂(g)?
Chemistry
1 answer:
mario62 [17]2 years ago
8 0

Answer:

Answer is in the attachment.

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The solubility of nitrogen gas at 25 ◦C and 1 atm is 6.8×10−4 mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm,
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Answer:

Concentration of dissolved nitrogen = 5.2 × 10⁻⁴ mol/L

Explanation:

More the pressure of the gas, more will be its solubility.

So, for two different pressure, the relation between them is shown below as:-

\frac {P_1}{C_1}=\frac {P_2}{C_2}

Given ,  

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C₁ = 6.8 × 10⁻⁴ mol/L

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Using above equation as:

\frac{1\ atm}{6.8\times 10^{-4}\ mol/L}=\frac{0.76\ atm}{C_2}

C_2=\frac{0.76\times 6.8\times 10^{-4}}{1}\ mol/L

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Did democritus belive atoms retain there identity as a chemical reaction
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No He believed tiny particles were invisible and couldn't be changed....So No The person that believed in this was Dalton .
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