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Suppose 1.20 ATM of CH4(g), 2.03 ATM of C2H6(g), and 15.69 ATM of O2(g) are placed in a flask at a given temperature. The reactions are given below.
CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g) KP = 1.0 104
2 C2H6(g) + 7 O2(g) 4 CO2(g) + 6 H2O(g) KP = 1.0 108
Calculate the equilibrium pressures of all gases.
PCH4
Enter a number with the correct number of significant figures.
1atm
PC2H6
Enter a number with the correct number of significant figures.
2atm
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What does Dalton's law of partial pressures?
The total pressure of a gas mixture is the sum of the individual pressures.
What is the total pressure of a gas mixture containing partial pressures of 0.23 ATM 0.43 ATM and 0.98 ATM?
According to Dalton's Law, the total pressure is the sum of the partial pressures of all gases present. Thus Ptotal = 0.23 atm + 0.43 atm + 0.98 atm = 1.64 atm
A mixture of gases contains 4.46 moles of neon Ne 0.74 moles of argon Ar and 2.15 moles of Xenon Xe Calculate the partial pressures of the gases if the total pressure is 2.00 ATM at a certa?
500
What are responsible for gas exchange in the lungs?
The partial pressures of each of the gasses, as present in the blood and in the alveoli.
What is the total pressure of a gas mixture containing partial pressures of 0.23 ATM ATM and 0.89 ATM?
1.54 atm
What three factors cause the partial pressures of gases in the alveoli to differ from pressures in the atmosphere?
You know, the factors of partial pressure
How does the total pressure of a mixture of gases relate to the partial pressures of the individual gases in a mixture?
total pressure = sum of all partial pressures.
What are the characteristics of partial pressure?
Dalton's law of partial pressures) states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases.
What law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of its individual gases?
The pressure of each gas in a mixture is called the partial pressure of that gas.
What does Dalton's law of partial pressures?
The total pressure of a gas mixture is the sum of the individual pressures.
What does Dalton's Law of Partial Pressures say?
The total pressure of a gas mixture is the sum of the individual pressures.
What is the partial pressure of a gas pressures in the mixture?
The partial pressure is the pressure exerted by just one gas in the mixture.
Does Dalton's law of partial pressures state that total pressure exerted by a mixture of gases is the sum of the pressures exerted independently by each gas in the mixture?
Yes. That is True. Dalton's Law is: that pressure exerted by a mixture of gases is the sum of the pressures exerted independently by each gas in the mixture. Reference: Human Anatomy and Physiology Marieb and Hoehn
Why do you express respiratory gas values in the body as partial pressures?
not sure
Who developed the concepts that the total pressure of a mixtures of gases is the sum of their partial pressures?
That's called Dalton's Law of Partial Pressures, which should give you a hint.
What is the total pressure of a gas mixture containing partial pressures of 0.23 ATM 0.43 ATM and 0.98 ATM?
According to Dalton's Law, the total pressure is the sum of the partial pressures of all gases present. Thus Ptotal = 0.23 atm + 0.43 atm + 0.98 atm = 1.64 atm
How does the total pressure of a mixture of gases relate to the partial pressure of the individual gases in a mixture?
total pressure = sum of all partial pressures.
