**Ideal Gas Law Calculation**If an ideal gas has a pressure of \(6.590 \times 10^5 \, \text{Pa}\), a temperature of \(43.00 \, ^\circ \text{C}\), and a volume of \(0.0127 \, \text{m}^3\), how many moles \(n\) of gas are in the sample?\(n =\) [Answer box]**Explanation:**To find the number of moles \(n\) of the gas, use the ideal gas law equation \(PV = nRT\), where:- \(P\) is the pressure,- \(V\) is the volume,- \(n\) is the number of moles,- \(R\) is the ideal gas constant (\(8.314 \, \text{J/mol·K}\)),- \(T\) is the temperature in Kelvin.Convert temperature from Celsius to Kelvin by adding 273.15. Calculate \(n\) using the rearranged equation \(n = \frac{PV}{RT}\).

Answered: Image /qna-images/answer/050765cf-07e2-4440-b19d-ca423c7d6664.jpg

Answered: If an ideal gas has a pressure of 6.590…

If an ideal gas has a pressure of 6.590 x 10° Pa, a temperature of 43.00 °C, and a volume of 0.0127 m², how many moles n of gas are in the sample? n = mol

College Physics

11th Edition

ISBN:9781305952300

Author:Raymond A. Serway, Chris Vuille

Publisher:Raymond A. Serway, Chris Vuille

Chapter1: Units, Trigonometry. And Vectors

Section: Chapter Questions

Problem 1CQ: Estimate the order of magnitude of the length, in meters, of each of the following; (a) a mouse, (b)...

See similar textbooks

Similar questions

An ideal gas at 17.4 °C and a pressure of 2.96 x 105 Pa occupies a volume of 3.86 m3. (a) How many moles of gas are present? (b) If the volume is raised to 4.93 m3 and the temperature raised to 30.4 °C, what will be the pressure of the gas?
A tank contains 10.6 g of chlorine gas (Cl₂) at a temperature of 84 °C and an absolute pressure of 6.00 × 105 Pa. The mass per mole of Cl2 is 70.9 g/mol. (a) Determine the volume of the tank. (b) Later, the temperature of the tank has dropped to 32 °C and, due to a leak, the pressure has dropped to 3.00 × 105 Pa. How many grams of chlorine gas have leaked out of the tank? (a) Number i (b) Number Units Units
Gas is confined in a tank at a pressure of 9.2 atm and a temperature of 27.0°C. If two-thirds of the gas is withdrawn and the temperature is raised to 65.0°C, what is the pressure of the gas remaining in the tank? atm
n = 3.9 moles of an ideal gas are pumped into a chamber of volume V = 0.125 m3. Part (a) The initial pressure of the gas is 1 atm. What is the initial temperature (in K) of the gas? Part (b) The pressure of the gas is increased to 10 atm. Now what is the temperature (in K) of the gas?
A gas chamber is to be designed to separate two gases with the following specifications: Hot gas temperature 1145°C Cold gas temperature 45°C Hot gas heat transfer coefficient 230 W/m² K Cold gas heat transfer coefficient 290 W/m² K Metal wall thermal conductivity 115 W/m K If the maximum temperature of the wall on the hot side does not exceed 545°C, using thermal resistance concept, what thickness should the metal wall between the hot gas and cold gas be in mm?
A hot air balloon uses the principle of buoyancy to create lift. By making the air inside the balloon less dense then the surrounding air, the balloon is able to lift objects many times its own weight. A large hot air balloon has a maximum balloon volume of 2090 m3 a. What is the density of air inside the balloon, in terms of the pressure P, temperature T, molar mass M, and the gas constant R? b. How much mass can this balloon lift (in addition to the mass of the gas inside) in terms the balloon volume Vb, the atmosphere air density ρa, the density of the air in the balloon ρg, and the gravitational acceleration g? c. If the air temperature in the balloon is 54 °C, how much additional mass, in kilograms, can the balloon lift? Assume the molar mass of air is 28.97 g/mol, the air density is 1.20 kg/m3, and the air pressure is 1 atm.
The volume of an automobile tire is 2.5 × 10−2m3 . the pressure of the air in the tire is 3 atm and the temperature is 37C ◦ . what is is the mass of air in grams ? The mean molecular mass of air is 29g. 1 atm = 1.01 × 105 Pa ; Calculate to 2 decimals.
The total translational kinetic energy of the molecules of a sample of gas at 415 K is 17500 J. How many moles n does the sample comprise? mol n = Find the average translational kinetic energy Ky of a single molecule. J Kav
If 86.5 moles of an ideal gas occupies 0.0275 cubic meters at 39.5 °C, what is the pressure of the gas? pressure: Pa
A 10.0 L container contains a certain gas at a temperature of 25.0◦C and pressure of 9.50 atm. Calculate the number of moles of gas in the container.
The absolute pressure inside an oxygen tank is P=100kPa, the temperature is 27°C, and the mass is m=3.0 kg. Assume the oxygen behaves as an ideal gas. The gas constant of oxygen is R=0.2598 kPa·m3/kg·K. The temperature relation is T(K)=T(°C)+273. Determine the volume of oxygen tank ______ m3
A 7.97 m3 tank contains 10.5 g of chlorine gas (Cl2) and an absolute pressure of 5.50 × 105 Pa. The mass per mole of Cl2 is 70.9 g/mol. (a) Determine the temperature of the tank in Celsius. (b) Later, the temperature of the tank has dropped to 33 °C and, due to a leak, the pressure has dropped to 3.30 × 105 Pa. How many grams of chlorine gas have leaked out of the tank?