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vladimir1956 [14]
3 years ago
8

A sample of three mixed gases is at 632.0 mmhg. if the partial pressure of co2 is 124.3 mmhg and the partial pressure of n2 is 4

61.9 mmhg, what is the partial pressure of o2?
Chemistry
2 answers:
Fantom [35]3 years ago
6 0

Answer:

45.8 mmhg

Explanation:

<em>According to Dalton's law of partial pressure, the total pressure of a gas mixture is the sum of the partial pressure of the individual gases that make up the mixture. </em>

Mathematically, the law can be expressed as:

P_{total} = P_1 + P_2 + ........ + P_n

In this case,

P_{total} = 632.0 mmhg,

P_{co2} = 124.3 mmhg

P_{N2} = 461.9

P_{O2} = ?

P_{total} = P_{co2} + P_{N2} + P_{O2}

                632.0 = 124.3 + 461.9 + P_{O2}

P_{O2} = 632.0 - + 124.3 + 461.9

                              = 45.8 mmhg

The partial pressure of O2 is 45.8 mmhg

goldfiish [28.3K]3 years ago
5 0
According to Dalton's Law of Partial pressures, the sum of the partial pressures of the individuals gas molecules that occupy a specific volume allows us to find the total pressure or find one of the partial pressures if the total pressure is known.

Partial pressure O2 = 632 - 124.3 - 461.9 = 45.8 mm Hg.
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Explanation:

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A: 2NO_(_g_) N_2_(_g_) + O_2_(_g_) ~Kc =\frac{1}{4.3x10^-^2^5}

Then if we add reactions A and B we can obtain the target reaction, so:

A: 2NO_(_g_) N_2_(_g_) + O_2_(_g_) ~Kc =\frac{1}{4.3x10^-^2^5}

B: 2NO_(_g_)+~O_2_(_g_)~2NO_2_(_g_)~Kc=6.4x10^9

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Kc=~1.49x10^+^3^4}

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