A jar contains a mixture of helium gas and krypton gas, with the sample containing equal masses of the two gases, \(m_{\text {sample, } \mathrm{He}}=m_{\text {sample,Kr }}\). Both gases are monatomic, they behave ideally, and the system is in equilibrium.

(a) What percentage of the pressure in the mixture is due to the helium? What percentage is due to the krypton?

(b) Explain why your answer in part \(a\) is reasonable. The atom masses are \(m_{\mathrm{He}}=6.646 \times 10^{-27} \mathrm{~kg}\) and \(m_{\mathrm{Kr}}=1.391 \times 10^{-25} \mathrm{~kg}\).