{"kind":"task","effective_mode":"full","benchmark":{"kind":"benchmark","effective_mode":"full","slug":"mmlu-pro","formal_name":"MMLU-Pro","introduction":"MMLU-Pro rebuilds MMLU with ten answer options instead of four and removes items that no longer separate models. Questions span fourteen academic and professional subjects.","introduction_ja":"","introduction_en":"","category":"Category not supplied","task_count":null,"acquisition_status":"Acquisition status not supplied","official_url":"https://huggingface.co/datasets/TIGER-Lab/MMLU-Pro","indexing_mode":"index","profile":{"resources":[],"task_format":"","scoring":"","metric":"","size":"","answer_access":"","license":"","citation":"","maintainer":"","released":"","why_hard":"","related":[],"history":"","construction":"","limitations":"","saturation":"","scores":[]}},"task_id":"bd471c71-631c-5280-861b-47c5325be1de","task_key":"default--test--4528","task_revision_id":"1","upstream_id":"4528","short_description":"Assume that all gases are perfect and that data refer to 298.15 K unless…","config":"default","split":"test","body":"{\"category\":\"chemistry\",\"options\":\"['+66.5$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+110.3$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+87.8$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+59.2$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+102.3$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+93.5$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+81.9$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+45.7$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+75.6$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$', '+125.4$\\\\\\\\mathrm{J} \\\\\\\\mathrm{K}^{-1} \\\\\\\\mathrm{~mol}^{-1}$']\",\"question\":\"Assume that all gases are perfect and that data refer to 298.15 K unless otherwise stated. The enthalpy of vaporization of chloroform $\\\\left(\\\\mathrm{CHCl}_3\\\\right)$ is $29.4 \\\\mathrm{~kJ} \\\\mathrm{~mol}^{-1}$ at its normal boiling point of $334.88 \\\\mathrm{~K}$. Calculate the entropy of vaporization of chloroform at this temperature.\",\"src\":\"scibench-atkins\"}","display_format":"text","language":"","answer_status":"published","assets":[],"source_url":"https://huggingface.co/datasets/TIGER-Lab/MMLU-Pro","history":"initial import","indexing_mode":"index","subproblems":[],"grids":[]}