Suppose you have 2.86 moles of an ideal gas. What is the average kinetic energy of that gas (in units of kJ) if the temperature of the gas is 279.1K?
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Suppose you have 2.86 moles of an ideal gas. What is the average kinetic energy of that gas (in units of kJ) if the temperature of the gas is 279.1K? Note: It is understood that the unit of your answer is some number of kilo-Joules, however do not explicitly include units in your answer. Enter only a number. If you do enter a unit ("kJ" in this case), you answer will be counted wrong.
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- The pressure, volume, and temperature of a mole of an ideal gas are related by the equation PV = 8.31T, where P is measured in kilopascals, V in liters, and T in kelvins. Use differentials to find the approximate change in the pressure if the volume increases from 10 L to 10.6 L and the temperature decreases from 335 K to 330 K. (Note whether the change is positive or negative in your answer. I Round your answer to ti decimal places.A cylinder containing 100.9 cubic centimeter of gas at a pressure of 376 kPa when its temperature is 534 K. Given that its temperature is unchanged when the pressure was increased by a factor of 5.9, Determine the new volume of the gas (In cubic centimeter). Note: Your answer must be in cubic centimeter, however, do not include the unit, just enter the magnitude that corresponds to the final volume in cubic centimeter. Round your answer to 2 decimal points Round your answer to 2 decimal pointsThe pressure, volume, and temperature of a mole of an ideal gas are related by the equation PV = 8.31T, where P is measured in kilopascals, V in liters, and T in kelvins. Use differentials to find the approximate change in the pressure (in kPa) if the volume increases from 11 L to 11.6 L and the temperature decreases from 370 K to 360 K. (Note whether the change is positive or negative in your answer. Round your answer to two decimal places.)
- A container holds 102.9 liters of Oxygen at 268.4K and a pressure of 1.95 atmospheres. How much heat is required to raise the temperature of this gas to 314.1K, holding the volume constant? Give your answer in kJ. Treat the gas as an ideal gas. Note: It is understood that your answer is in units of kilo-Joules, however do not explicitly include units in your answer. Enter only a number. If you do enter a unit ("kJ" in this case), you answer will be counted wrong.In a hypothetical diesel engine the fuel is compressed from 528mL to 39.7 mL. This rasies the temperature of the fuel form 25°C to its ignition temperature of 210°C. If the fuel begins at 1.00atm, what is the pressure of the fuel at its ignition temperature.? Express your answer to 1 decimal place. Be sure to use the proper abbreviation of the UNITSPROBLEMS 1.1. In the table below, a number in the top row represents the pressure of a gas in the bulb of a constant-volume gas thermometer (corrected for dead space, thermal expansion of bulb, etc.) when the bulb is immersed in a water triple-point cell. The bottom row represents the corresponding readings of pressure when the bulb is surrounded by a material at a constant unknown temperature. Calculate the ideal- gas temperature T of this material. (Use five significant figures.) PTP, kPa P, kPa 133.32 99.992 33.331 66.661 102.37 204.69 153.54 51.190
- Suppose you have 0.53 moles of an ideal gas. What is the average kinetic energy of that gas (in units of kJ) if the temperature of the gas is 280.2K? Note: It is understood that the unit of your answer is some number of kilo-Joules, however do not explicitly include units in your answer. Enter only a number. If you do enter a unit ("kJ" in this case), you answer will be counted wrong.The ideal gas law describes the state of a hypothetical ideal gas, i.e., PV = nRT where P is the pressure in Pascal, V is the volume in liters L, R is the ideal gas constant, T is the temperature in kelvin K, and n is the amount of substance. Suppose a researcher has n = 0.654 moles of neon gas. He observed that T and V are increasing at rates of 3 K/min and 2 L/min, respectively, using the fixed gas constant R= 8.31 J/K.mol, find the rate at which the pressure is changing when V = 12.3 L and T = 447K.Pump some air into the container and hold the volume constant.Heat the gas using the heater under the container. temperature(K) pressure(kPa) 400 800 500 1000 600 1200 700 1400 800 1600 900 1800 1)Plot a graph of Pressure vs temperature and attached the graph below (show the data points and label the axes) 2)find the “molar density” of the gas in the container. (unit of answer: mole/m3)(Hint: consider the ideal gas law , the graph should be ??=??? a straight line, you can use the slope of the graph to find the answer. Pay attention to the unit. R=ideal gas constant=8.314 JK-1mol-1=8.314 m3PaK-1mol-1) Include the appropriate units in the physical quantities.(with steps)
- If you have 4 moles of a diatomic ideal gas (such as oxygen or nitrogen), how much heat is required to raise the temperature of this gas from 269.5K to 288.3K if the volume of the gas remains constant during the heating? Note: It is understood that your answer is in units of Joules, however do not explicitly include units in your answer. Enter only a number. If you do enter a unit ("J" in this case), you answer will be counted wrong.A bottle of volume V = 0.15 m³ contains helium gas (a monatomic gas) at a pressure p = 722,266 Pa (Pascal = N/m² and temperature T = 300 K. Calculate a numerical value for the internal energy U of this gas. Include units in your answer, using Sl units (m for meters, kg for kilograms, s for seconds, J for joules, K for kelvin, etc.). Write your answer as an exponential as described in the instructions.Ideal gases are often studied at standard ambient temperature and pressure (SATP). The International Union of Pure and Applied Chemistry (IUPAC) defines SATP to be T = 25° C and P = 100 kPa. a. Calculate N/V (in particles per cubic meter) for an ideal gas at SATP b. How many atoms of an ideal gas at SATP are there in one cubic centimeter?