A gas mixture for use in some lasers contains 5.00% by weight HCl, 1.00% H2, and 94% Ne. The mixture is sold in cylinders that have a volume of 49.0 L and a pressure of 13,900 kPa at 210 °C. What is the partial pressure in kilopascals of each gas in the mixture?

a) HCl: 695 kPa, H2: 139 kPa, Ne: 13,066 kPa
b) HCl: 695 kPa, H2: 1,390 kPa, Ne: 12,066 kPa
c) HCl: 695 kPa, H2: 1,390 kPa, Ne: 13,066 kPa
d) HCl: 1,390 kPa, H2: 695 kPa, Ne: 13,066 kPa

Using Dalton's law of partial pressure, the partial pressures of HCl, H₂, and Ne in a gas mixture are calculated as 695 kPa for HCl, 139 kPa for H₂, and 13,066 kPa for Ne, matching option (a).

To calculate the partial pressures of each gas in the mixture, we will utilize Dalton's law of partial pressure. According to Dalton's law, the total pressure of a mixture of gases is equal to the sum of the partial pressures of all the individual gases in the mixture.

The partial pressure of a gas in a mixture is the pressure that gas would exert if it were alone in the container.

Given that the total pressure in the cylinder is 13,900 kPa, we can calculate the partial pressure of each component by multiplying the total pressure by the percentage (by weight) of each gas in the mixture.

HCl partial pressure = Total pressure x percentage of HCl = 13,900 kPa x 0.05 = 695 kPa
H₂ partial pressure = Total pressure x percentage of H₂ = 13,900 kPa x 0.01 = 139 kPa
Ne partial pressure = Total pressure x percentage of Ne = 13,900 kPa x 0.94 = 13,066 kPa

We can see that the correct partial pressures for the gases in the mixture are HCl: 695 kPa, H₂: 139 kPa, and Ne: 13,066 kPa, which corresponds with option (a).