The partial pressure of gas C is 0.54atm. The correct option is D.
<h3>What is partial pressure?</h3>
The pressure that one of the gases in a mixture would exert if it were in the same volume on its own.
The total pressure of A, B and C is 6.11 atm.
The partial pressure of A is 1.68 atm
The partial pressure of B is 3.89 atm.
Total pressure = sum of partial pressures of all the gasses in that mixture
6.11atm = 1.68atm + 3.89atm + Pc
Pc = 6.11atm - (1.68 + 3.89) = 0.54atm
Thus, the partial pressure of C is 0.54atm. The correct option is D.
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Explanation:
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Answer:
Explanation:
<u>1. Chemical equation (given)</u>
<u>2. Chemical equation with the phases:</u>
<u>3. Equilibrium constant</u>
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Only the species in aqueous phase appear in the equilibrium constant.
<u>4. Calculate Kb</u>
<u>5. Write the ICE (initial, change, equilibrium) table for the aqueous species</u>
ICE table:
C₅H₅N C₅H₅NH⁺ +OH⁻
Initial 0.345M 0 0
Change - x + x + x
Equilibrium 0345 - x x x
<u>5. Substitute in the equilibrium constant</u>
To solve you can neglect x in 0.345 - x, because x is much (very much) less than 0.345M.
<u>6. Calculate pOH</u>
- pOH = - log [OH⁻] = - log (x) = -log (2.477 × 10⁻⁵) = 4.61
<u>7. Calculate pH</u>
- pH = 14 - pOH = 14 - 4.61 = 9.39
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