181 ml of hydrogen gas, measured at 24°c and 2.9 atm pressure, and 256 ml of nitrogen gas, measured at 24°c and 1.3 atm pressure, were forced into the 181 ml container at 24°c, what would be the pressure of the mixture of gases now in the 181 ml container?

To find the pressure of the mixture of gases in the 181 ml container, we can use the ideal gas law equation PV = nRT. By substituting the given values into the equation, we find that the pressure is 1.95 atm.

Explanation:

To calculate the pressure of the mixture of gases in the 181 ml container, we can use the ideal gas law equation: PV = nRT. Where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to convert the temperature from Celsius to Kelvin by adding 273.15. Then, we can calculate the pressure using the equation:

P = (n1 * P1 + n2 * P2) / V

In this case, since the volume is the same for both gases, we can simplify the equation:

P = (n1 * P1 + n2 * P2) / V = (181 ml * 2.9 atm + 256 ml * 1.3 atm) / 181 ml = 1.95 atm.

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