Equal weight of methane and hydrigen are mixed in an empty container at 25°C. The fraction of the total pressure exerted by hydrogen is
discussed here:
http://www.jiskha.com/display.cgi?id=1412345782
That answer gives 1/9 for H2. The fraction for H2 is 8/9. See the post above http://www.jiskha.com/index.cgi? for the correct solution.
To determine the fraction of the total pressure exerted by hydrogen, we need to first understand the concept of partial pressure.
According to Dalton's law of partial pressures, the total pressure of a mixture of gases is equal to the sum of the partial pressures of each individual gas. The partial pressure of a gas is the pressure it would exert if it occupied the same space alone at the same temperature.
In this case, we have equal weights of methane and hydrogen. Since the molar mass of methane (CH4) is 16 g/mol and the molar mass of hydrogen (H2) is 2 g/mol, we can conclude that there are 8 times more moles of methane than hydrogen in the mixture.
Let's assume we have 8 moles of methane (CH4) and 1 mole of hydrogen (H2). We can also assume that the total pressure of the mixture is 1 atmosphere (atm) at 25°C.
Now, to find the partial pressure of hydrogen, we need to express the moles of hydrogen as a fraction of the total moles, and then multiply it by the total pressure.
Moles of hydrogen (H2) = 1
Moles of methane (CH4) = 8
Total moles = moles of hydrogen + moles of methane
Fraction of hydrogen pressure = (moles of hydrogen / total moles) * total pressure
Fraction of hydrogen pressure = (1 / (1 + 8)) * 1 atm
Fraction of hydrogen pressure = (1 / 9) * 1 atm
Therefore, the fraction of the total pressure exerted by hydrogen in the mixture is approximately 1/9 or 0.111 atm.
Note: The actual weight or moles of methane and hydrogen could vary, but the concept and calculations would remain the same.