A balloon at the top of Mount Logan occupies a volume of 775mL at a temperature of -28°C and a pressure of 92.5kPa. What is the pressure at the bottom of the mountain if the same balloon has a volume of 825mL at a temperature of 15°C?
-28oC = 273 - 28 = 245 K
15oC = 273 + 15 = 288 K
According to the combined gas law,
"\\frac{p_1V_1}{T_1}=\\frac{p_2V_2}{T_2}"
Therefore,
"p_2=\\frac{p_1V_1T_2}{T_1V_2}=\\frac{92.5kPa\\times775mL\\times288K}{245K\\times825mL}=102kPa"
Answer: 102 kPa
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