**Problem Statement:**An automobile tire is filled with air at a pressure of 27.0 lb/in² at 25°C. A cold front moves through and the temperature drops to 5°C. Assuming no change in volume, what is the new tire pressure?**Explanation:**This problem involves the relationship between pressure and temperature in gases, known as Gay-Lussac's Law. The law states that the pressure of a gas is directly proportional to its absolute temperature when volume remains constant. The formula is:\[ P_1/T_1 = P_2/T_2 \]Where:- \( P_1 \) = initial pressure- \( T_1 \) = initial temperature in Kelvin- \( P_2 \) = final pressure- \( T_2 \) = final temperature in Kelvin**Solution Steps:**1. Convert temperatures from Celsius to Kelvin: - \( T_1 = 25°C + 273.15 = 298.15 K \) - \( T_2 = 5°C + 273.15 = 278.15 K \)2. Use the formula \[ P_1/T_1 = P_2/T_2 \] to solve for \( P_2 \): - Rearrange to find \( P_2 \): \[ P_2 = P_1 \times (T_2/T_1) \] - Substitute known values: \[ P_2 = 27.0 \, \text{lb/in}^2 \times \left(\frac{278.15}{298.15}\right) \]3. Calculate \( P_2 \).Thus, the new tire pressure can be calculated based on the provided initial conditions and the temperature change.

The ideal gas is noticed to follow PV=nRT. The real gases are assumed to depict the same behaviour. The pressure of the (ideal) gas is proportional to the temperature, and number of moles of the gas. Whereas, lesser volume creates more pressure. Expansion releases the pressure. All the calculations are made with the standard units of each parameter.

Science

Chemistry

An automobile tire is filled with air at a pressure of 27.0 lb/in² at 25°C. A cold front moves through and the temperature drops to 5°C. Assuming no change in volume, what is the new tire pressure?

An automobile tire is filled with air at a pressure of 27.0 lb/in² at 25°C. A cold front moves through and the temperature drops to 5°C. Assuming no change in volume, what is the new tire pressure?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A 1.20 L weather balloon on the ground has a temperature of 25.0°C and is at atmospheric pressure (1.00 atm). When it rises to an elevation where the pressure is 0.740 atm, then the new volume is 1.80 L. What is the temperature (in °C) of the air at this elevation?
An “empty" spray can contains residual propellant gas that has a pressure of 772 torr at 23°C. The can is then heated to 475 °C. (a) What is the gas pressure in the hot can if the volume remains constant? (b) What is the gas pressure in the hot can if the can slightly expands during heating and its volume increases by 6.50%?
A sample of methane occupied 18.95 L at 41.03 °C. When the volume changed to 11.60 L at 16.59 °C, the pressure was 2.044 atm. Calculate the original pressure (atm). Write out the problem on paper in order to answer the questions related to the setup and the calculation for this problem. Identify all of the terms in this problem and enter the numerical values (without units) in the appropriate blanks. Convert temperature(s) to K, and enter with proper s.f. If the term doesn't apply in this problem enter 0. Enter a question mark for the variable being calculated. Do not leave any blank empty. P1 = V1 = T1= n1= P2= V2= T2= n2= Rearrange the gas law equation needed to solve for the variable of interest. Identify which terms are in the numerator and which terms are in the denominator after rearranging. Do not leave any blank empty. Enter a zero "0" if the blank is not needed. Use the following abbreviations: pressures = P1, P2; volumes = V1, V2; temperatures = T1, T2, moles = n1, n2…
Using these formulas pressure at sea level =760 mmHg and P1V1=P2V2
What is the pressure of the air, in atmatm, in the lungs when the gas expands to 150.0 mLmL at a body temperature of 37 ∘C∘C, and the amount of gas remains constant?
1
After 0.600 L of Ar at 1.19 atm and 240.0 °C is mixed with 0.200 L of O₂ at 428. torr and 110.0 °C in a 400.- mL flask at 28.0 °C, what is the pressure in the flask? Be sure your answer has the correct number of significant figures. Note: Reference the Conversion factors for non-SI units, Fundamental constants and SI prefixes tables for additional information. atm
A weather balloon is inflated with helium to a volume of 685 L at sea level, where the temperature is 30°C and the barometric pressure is 760. torr. The balloon rises to an altitude of 4500 feet where the pressure is 645 torr and the temperature is 6°C. What is the change in volume (in liters) of the balloon in going from sea level to 4500 feet?
Calculate the isoionic and isoelectric pH of 0.01111 M methionine. Enter your answers to the hundredths place. isoionic pH = 1 X100 TOOLS x10⁰ isoelectric pH = 2.089 x10-6 Amino Acid Asparagine Glutamine Isoleucine Leucine Methionine Phenylalanine Proline Serine Tryptophan Valine. pKal 2.16 2.19 2.318 2.328 2.18 2.20 1.952 2.187 2.37 2.286 pK₂2 8.73 9.00 9.758 9.744 9.08 9.31 10.640 9.209 9.33 9.719
A balloon is inflated to a volume of 7.0 L on a day when the atmospheric pressure is 765 mmHg. The next day, as a storm front arrives, the atmospheric pressure drops to 727 mmHg. Assuming the temperature remains constant, what is the new volume of the balloon, in liters? V = L
An airplane is pressurized with air to 660 mmHg. If air is 21% oxygen, what is the partial pressure of oxygen on the plane? If the partial pressure of oxygen drops below 105 mmHg, passengers become drowsy. If this happens, oxygen masks are released. What is the total cabin pressure at which oxygen masks are dropped?
The gas of a certain volcano had the following composition in mole percent: 60.0% CO2, 28.0% H2, 7.40% HCl, 1.80% HF, 2.70% SO2, and 0.100% H2S. What would be the partial pressure of HF in atmospheres if the total pressure was 285 mmHg? 1atm = 760mmHg