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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
What else can I help you with?
How do you calculate Kp from partial pressures?
To calculate Kp from partial pressures, you use the formula Kp (P products)(coefficients of products) / (P reactants)(coefficients of reactants), where P represents the partial pressures of the substances involved in the reaction.
How do you calculate the equilibrium constant Kp for a chemical reaction?
To calculate the equilibrium constant Kp for a chemical reaction, you need to determine the partial pressures of the reactants and products at equilibrium. Then, you can use these values to set up the expression for Kp, which is the ratio of the product of the partial pressures of the products to the product of the partial pressures of the reactants, each raised to the power of their respective stoichiometric coefficients in the balanced chemical equation.
How can one determine the equilibrium constant, Kp, from partial pressures in a chemical reaction?
To determine the equilibrium constant, Kp, from partial pressures in a chemical reaction, you can use the formula Kp (P products)(coefficients of products) / (P reactants)(coefficients of reactants). This involves taking the partial pressures of the products and reactants at equilibrium and plugging them into the formula to calculate the equilibrium constant.
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?
To determine the partial pressures of each gas, you first need to calculate the mole fraction of each gas in the mixture. Then, you can find the partial pressure by multiplying the mole fraction of each gas by the total pressure. Finally, the partial pressures would be: Ne = 0.446 atm, Ar = 0.074 atm, and Xe = 0.28 atm.
The gases in a mixture have the following partial pressures at the same volume and temperature 10.13 kPa nitrogen 720 mm argon 1.25 ATM of helium 780 torr oxygen and 0.92 ATM of carbon dioxide What?
To calculate the total pressure of the mixture, you need to convert all the partial pressures to a single unit. Let's convert all the partial pressures to ATM: 1 kPa = 0.00986923 ATM, 1 mmHg = 0.00131579 ATM, and 1 torr = 0.00131579 ATM. Then add all the partial pressures together to get the total pressure of the mixture.
How do you calculate Kp from partial pressures?
To calculate Kp from partial pressures, you use the formula Kp (P products)(coefficients of products) / (P reactants)(coefficients of reactants), where P represents the partial pressures of the substances involved in the reaction.
How do you calculate the equilibrium constant Kp for a chemical reaction?
To calculate the equilibrium constant Kp for a chemical reaction, you need to determine the partial pressures of the reactants and products at equilibrium. Then, you can use these values to set up the expression for Kp, which is the ratio of the product of the partial pressures of the products to the product of the partial pressures of the reactants, each raised to the power of their respective stoichiometric coefficients in the balanced chemical equation.
How can one determine the equilibrium constant, Kp, from partial pressures in a chemical reaction?
To determine the equilibrium constant, Kp, from partial pressures in a chemical reaction, you can use the formula Kp (P products)(coefficients of products) / (P reactants)(coefficients of reactants). This involves taking the partial pressures of the products and reactants at equilibrium and plugging them into the formula to calculate the equilibrium constant.
Atmospheric pre contains 20 o2 and80 n2 exert pressure of 760 mm.calculate partial press of both gas?
To calculate the partial pressures of oxygen (O₂) and nitrogen (N₂) in the atmosphere, you can use Dalton's Law of Partial Pressures. The total pressure is 760 mmHg. The partial pressure of O₂ is 20% of 760 mmHg, which is 152 mmHg, and the partial pressure of N₂ is 80% of 760 mmHg, which is 608 mmHg. Therefore, the partial pressures are 152 mmHg for O₂ and 608 mmHg for N₂.
A mixture of He Ne and N2 gases has a pressure of 1.943 ATM. If the pressures of He and Ne are 0.137 ATM and 0.566 ATM respectively what is the partial pressure of N2 in the mixture?
To find the partial pressure of N2 in the mixture, we can use Dalton's Law of partial pressures, which states that the total pressure is the sum of the partial pressures of the individual gases. Given the total pressure (1.943 ATM) and the partial pressures of He (0.137 ATM) and Ne (0.566 ATM), we can calculate the partial pressure of N2 as follows: Partial pressure of N2 = Total pressure - (Partial pressure of He + Partial pressure of Ne) Partial pressure of N2 = 1.943 ATM - (0.137 ATM + 0.566 ATM) = 1.943 ATM - 0.703 ATM = 1.240 ATM. So, the partial pressure of N2 is 1.240 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?
To determine the partial pressures of each gas, you first need to calculate the mole fraction of each gas in the mixture. Then, you can find the partial pressure by multiplying the mole fraction of each gas by the total pressure. Finally, the partial pressures would be: Ne = 0.446 atm, Ar = 0.074 atm, and Xe = 0.28 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
What is the partial pressure of oxygen if the partial pressures of the nitrogen and carbon dioxide are 100 kPA and 24 kPa respectively?
To find the partial pressure of oxygen, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of all gases in a mixture. Assuming the total pressure is the sum of the given partial pressures, you can calculate it as follows: Total Pressure = Partial Pressure of Nitrogen + Partial Pressure of Carbon Dioxide + Partial Pressure of Oxygen. If we denote the partial pressure of oxygen as ( P_O ): Total Pressure = 100 kPa + 24 kPa + ( P_O ). Without the total pressure, we cannot determine the exact value of the partial pressure of oxygen. However, if the total pressure is known, you can rearrange the equation to solve for ( P_O ) as ( P_O = \text{Total Pressure} - 124 kPa ).
The gases in a mixture have the following partial pressures at the same volume and temperature 10.13 kPa nitrogen 720 mm argon 1.25 ATM of helium 780 torr oxygen and 0.92 ATM of carbon dioxide What?
To calculate the total pressure of the mixture, you need to convert all the partial pressures to a single unit. Let's convert all the partial pressures to ATM: 1 kPa = 0.00986923 ATM, 1 mmHg = 0.00131579 ATM, and 1 torr = 0.00131579 ATM. Then add all the partial pressures together to get the total pressure of the mixture.
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.
