Concept explainers
(a)
The graph of length versus temperature for mercury.
Given:
The length of column of mercury in the thermometer is 4 cm .
The pressure of water is 1 atm
The length of column of mercury in the thermometer is 4 cm .
The thermometer in the boiling water is 24 cm .
Introduction:
Explanation:
The graph of length of the mercury column versus temperature is:
The equation for the graph is:
L = m T + C
Here, L is the length in cm , T is the temperature in Celsius and C is the intercept.
Substitute 0.200 cm / °C for m and 4.0 cm for C in equation (1).
L = ( 0.200 cm / °C ) T + 4.0 cm
Conclusion:
The graph of length versus temperature for mercury.
Given:
The length of column of mercury in the thermometer is
The pressure of water is
The length of column of mercury in the thermometer is
The thermometer in the boiling water is
Introduction:
Explanation:
The graph of length of the mercury column versus temperature is:
The equation for the graph is:
Here,
Substitute
Conclusion:
(b)
The length of the column when the temperature is
(b)
The temperature when the length of the mercury column is
Want to see the full answer?
Check out a sample textbook solutionChapter 17 Solutions
One Semester Webassign Access Code for Tipler Physics for Scientists and Engineers
- At 25.0 m below the surface of the sea, where the temperature is 5.00C, a diver exhales an air bubble having a volume of 1.00 cm3. If the surface temperature of the sea is 20.0C, what is the volume of the bubble just before it breaks the surface?arrow_forwardAssuming the human body is primarily made of water, estimate the number of molecules in it. (Note that water has a molecular mass of 18 g/mol and there are roughly 1024 atoms in a mole)arrow_forwardA bubble of air is rising from the sea floor, from a depth of about 500 m. At this depth the pressure is 5.1*106 Pa (about 50.3 atm) and is at a temperature of about 7.0° C. It rises to the surface with the atmosphere, at a temperature of 20° C. If the bubble is observed to have a volume of 4 cm³ at the surface, what was its volume at the sea floor? Assume the number of moles of gas in the bubble is constant. B.arrow_forward
- A balloon is filled with helium gas at atmospheric pressure (1 atm) until its volume is 800 m3. The helium gas is then transferred to cylinders that have a volume of 2.3 m3 at a pres- sure of 13.3 atm. Calculate the number of cylinders used. Assume that the temperature of the helium gas remains constant. (1 atm = 1.013 × 105 Pa).arrow_forwardAssuming the human body is primarily made of water, estimate the number of molecules in it. (Note that water has a molecular mass of 18 g/mol and there are roughly 1024 atoms in a mole.)arrow_forwardA cylinder of gas at room temperature (20°C) has a pressure p1. To what temperature in degrees Celsius would the temperature have to be increased for the pressure to be 1.2p1?arrow_forward
- A Fahrenheit and a Celsius thermometer are both immersed in a fluid. a) If the two numerical readingsare identical, what is the temperature of the fluid expressed in ºK and ºR. b) If the Fahrenheittemperature is numerically twice that of the Celsius reading, what is the temperature of the fluidexpressed in ºK and ºR?arrow_forwardLarge helium-filled balloons are used to lift scientific equipment to high altitudes. (a) What is the pressure inside such a balloon if it starts out at sea level with a temperature of 10 °C and rises to an altitude where its volume is twenty times the original volume and its temperature is -40 °C? P2 = atm (b) What is the gauge pressure? (Assume atmospheric pressure is constant.) Gauge pressure: atmarrow_forwardIf a 5 m3 of gas initially at STP is placed under a pressure of 3 atm, the temperature of the gas rises to 17◦C. What is the volume now? Calculate to 2 decimals.arrow_forward
- The tidal lung volume of human breathing, representing the amount of air inhaled and exhaled in a normal breath, is 500 cm³. (Assume atmospheric pressure.) (a) What is the number of molecules of air inhaled with each human breath when the air temperature is 25.0°C? molecules (b) If the molar mass of air is 28.96 g/mol, what is the mass (in g) of air molecules inhaled with each breath? (Assume the air temperature is 25.0°C.) g (c) It has been calculated that all of the air in Earth's atmosphere could be collected into a sphere of diameter 1,999 km at a pressure of 1.00 atm. What is the mass (in kg) of the air in Earth's atmosphere? (Assume the density of air used in this calculation was 1.225 kg/m³.) kg (d) If all 7 billion humans on Earth inhaled simultaneously, what percentage of the atmosphere would be inhaled during this process? (Assume the air temperature is 25.0°C everywhere on Earth.) %arrow_forwardThe pressure P (in kilopascals), volume V (in liters), and temperature T (in kelvins) of a mole of an ideal gas are related by the equation PV = 8.317. Find the rate at which the volume is changing when the temperature is 325 K and increasing at a rate of 0.05 K/s and the pressure is 29 and increasing at a rate of 0.07 kPa/s. Please show your answers to at least 4 decimal places. dV dt L/sarrow_forwardWhen the coefficient of linear expansion, a, and the temperature change, T-T, are large, a length L, of a solid substance expands in length to a(T, -T₂) L₁ = L₁e O L=L[1 + a(Tƒ– T;)]. ○ Ly=al (Ty-T). O L=L[1 + In(a(T₁-T))]. a(T, I₂ = ₁₂₁[ 1 + ª²(²₁-7)].arrow_forward
- Physics for Scientists and Engineers: Foundations...PhysicsISBN:9781133939146Author:Katz, Debora M.Publisher:Cengage LearningUniversity Physics Volume 1PhysicsISBN:9781938168277Author:William Moebs, Samuel J. Ling, Jeff SannyPublisher:OpenStax - Rice UniversityPrinciples of Physics: A Calculus-Based TextPhysicsISBN:9781133104261Author:Raymond A. Serway, John W. JewettPublisher:Cengage Learning