The excess internal energy of
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Chapter 11 Solutions
COLLEGE PHYSICS,V.1-W/ENH.WEBASSIGN
- For divers going to great depths, the composition of the air in the tank must be modified. The ideal composition is to have approximately the same number of O2 molecules per unit volume as in surface air (to avoid oxygen poisoning), and to use helium instead of nitrogen for the remainder of the gas (to avoid nitrogen narcosis, which results from nitrogen dissolving in the bloodstream). Of the molecules in dry surface air, 78.0% are N2, 21.0% are O2, and 1.00% are Ar. (Assume that the density of seawater is 1025 kg/m3 and the temperature is 20.0°C.) Density of dry air at 20.0°C is 1.20 kg/m3. Molar mass of N2 is 14.007 g/mol, O2 is 15.999 g/mol, and Ar is 39.948 g/mol. For a diver going to a depth of 141 m, what percentage of the gas molecules in the tank should be O2?arrow_forwardA highway is made of concrete slabs that are 16.2 m long at 20.0°C. Expansion coefficient of concrete is α = 12.0 × 10−6 K−1. A) If the temperature range at the location of the highway is from −20.0°C to +36.9°C, what size expansion gap should be left (at 20.0°C) to prevent buckling of the highway? in mm B) If the temperature range at the location of the highway is from −20.0°C to +36.9°C, how large are the gaps at −20.0°C? in mmarrow_forwardUse the ideal gas law, “PV= nRT”, and the universal gas constant R = 0.0821 L*atm/K*mol to solve the following problems: If pressure is needed in kPa then convert by multiplying by 101.3 kPa / 1atm to get R =8.31 L*kPa / (K*mole) KINDLY solve it with solutions 12)If I have 72 liters of gas held at a pressure of 3.4 atm and a temperature of 225 K, how many moles of gas do I have?arrow_forward
- Total lung capacity of a typical adult is approximately 5.0 L. Approximately 20% of the air is oxygen. At sea level and at an average body temperature of 37°C, how many moles of oxygen do the lungs contain at the end of an inhalation?arrow_forwardWhen you take a normal breath of air, you typically inhale 4.43 x10-4 m3 of air. Assuming that the air has an oxygen content of 20.82%, the pressure in the lungs is 1.083 x105 Pa and that air is an ideal gas at a temperature of 298.3 K, find the number of oxygen molecules in a normal breatharrow_forwardAt sea level and at a body temperature of 37 degrees Celsius, how many oxygen molecules do the lungs contain at the end of a strong inhalation? (Hint: answer is not 0.039 molecules) Use Avogadro’s number to calculate the answer.arrow_forward
- A highway is made of concrete slabs that are 12.2 m long at 20.0°C. Expansion coefficient of concrete is α = 12.0 × 10−6 K−1. If the temperature range at the location of the highway is from −20.0°C to +32.7°C, what size expansion gap should be left (at 20.0°C) to prevent buckling of the highway? answer has to be in mm.arrow_forward1. on a hot summer day the temperature is 40.0°c and the pressure is 1.01x10^5 Pa. et us model the air as all nitrogen of molecular mass 28.0g/mol having molecules of diamtere 0.500 nm (nano = 10^-9) that are moving at their root-mean-square speed. Avogadro's number is 6.02x10^23 molecules/mol, the ideal gas constant is 8.31 J/mol . K, and the boltzmann constant is 1.38x10^-23 J/K calculate reasonable estimates for A. the root mean-square speed of the nitrogen molecules B. the average distance of a typical molecule travels between collisions C. the average time a molecule travels between collisions, assuming that the molecules are moving at their root-mean-swuare speeds D. the molecule of collisions an average molecule undergoes per second 2. A 648-G Empty Iron Kettle Is Put On A Stove. How Much Heat, In Joules, Must It Absorb To Raise Its Temperature From 15.0°C To raise its temperature from 15°c to 37°c (the specific heat for iron is 113 ca;/g°C, 1 cal = 9.190J)arrow_forwardA weather balloon contains 12.0 m3 of hydrogen gas when the balloon is released from a location at which the temperature is 22.0°C and the pressure is 101 kPa. The balloon rises to a location where the temperature is -30.0°C and the pressure is 20.0 kPa. If the balloon is free to expand so that the pressure of the gas inside is equal to the ambient pressure, what is the new volume of the balloon? Assume that in both cases the hydrogen gas is in thermal equilibrium with the outside air.arrow_forward
- Use the ideal gas law, “PV= nRT”, and the universal gas constant R = 0.0821 L*atm/K*mol to solve the following problems: If pressure is needed in kPa then convert by multiplying by 101.3 kPa / 1atm to get R =8.31 L*kPa / (K*mole) KINDLY solve it with solutions 11 and 12 thank you 11)If I have 0.275 moles of gas at a temperature of 75 K and a pressure of 1.75 atmospheres, what is the volume of the gas? 12)If I have 72 liters of gas held at a pressure of 3.4 atm and a temperature of 225 K, how many moles of gas do I have?arrow_forwardFind the density of air at 0°C and 1.013 x10^5 Pa. One mole of air may be assumed to be 79% nitrogen (M=28.0 g) and 21% oxygen (M=32.0 g).arrow_forwardThe vapor pressure of water at 40.0oC is 7.34 X 103 N/m2. Using the ideal gas law, calculate the density of water vapor in g/m3 that creates a partial ressure equal to this vapor pressure. The result should be the same as the saturation vapor density at that temperature (51.1 g/m3)arrow_forward
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