How much heat will be absorbed by a 38.7 g piece of aluminum (specific heat = 0.930 J/g · °C) as it changes temperature from 23.0°C to 67.0°C? A sample of helium is initially at 515 torr in a volume of 2.85 L. a) If this sample of helium is at 24.7 °C, then how many moles of helium are present? b) What is the density of this gas sample at 24.7 °C? c) Suppose instead of helium you had a sample of argon gas at 24.7 °C. How many moles of argon would be present with the same pressure and volume? d) What would be the density of the argon gas sample at 24.7 °C? e) Which one of the following best explains why the densities are different? What is the mass of 5.00 L of H2O at STP? Two moles of nitrogen gas at 25°C, confined within a cylinder by a piston maintaining a constant pressure of 1 atm, is heated with 3.90 kJ of energy. Assume all the energy is used to do work of expansion of the gas at 1 atm. What will be the final temperature of the gas? Recall ?H = ?E + P?V and watch your units!
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Heat absorbed by aluminum: We can use the formula for heat absorbed: $q = mc\Delta T$, where $q$ is the heat absorbed, $m$ is the mass, $c$ is the specific heat, and $\Delta T$ is the change in temperature. Show more…
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