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1. What was the initial temperature of a gas contained in a 2.0-L bottle at a pressure of 1.00 atm if it was placed under vacuum and its pressure was reduced to 0.82 atm at a temperature of 10.0º C? Assume volume remains constant.
Feb 6, 2019

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Solution (partial):

$$\text {The equation for combined gas laws: }\\ \dfrac{P_1V_1}{T_1} = \dfrac{P_2V_2}{T_2}\\ \text { }\\ \text {The solution requires simple algebraic operations for this setup: }\\ \text { }\\ \dfrac{1.00 atm*2.00 L}{T_1} = \dfrac{0.82atm*2.00L}{10 C} \quad | \quad \text {solve for } T_1\\ \text { }\\ \text {Algebra 1 & 2 is prerequisite for chemistry; you should already have these skills. }\\ \text { }\\ \text {Post your (attempted) solution below. Someone will check it for you. }\\$$

GA

Feb 6, 2019
edited by GingerAle  Feb 6, 2019