Question

Let us first examine the behavior of an ideal gas when we force the volume to be a value of our choosing. We can examine how changes to the absolute temperature and number of moles affect the pressure of the gas particles (by selecting pressure with Rspd such that pressure cannot be controlled). Assume that 0.03 mol of helium at a temperature of 275.00 K occupy a volume of 1.40 L. Use the Run Experiment tool in the Simulation to determine the initial pressure of the gas and the new pressure values when the temperature or number of moles is changed to complete the following statements. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. ► View Available Hint(s) Reset Help 1.13 atm The initial pressure of the helium gas is inverse 0.52 atm From the initial conditions (0.03 mol and 275.00K), if you increased the amount of helium to 0.07 mol, the new pressure would be . Therefore, pressure 0.48 atm with the number of moles in proportion decreases increases From the initial conditions (0.03 mol and 275.00K), if you increased the temperature by 80.00 K, the new pressure would be . Therefore, pressure with temperature in proportion. direct 0.28 atm 1.29 atm 1.46 atm 0.62 atm

Answer 1

Let us first examine the behavior of an ideal gas when we force the volume to be a value of our choosing. We can examine how changes to the absolute temperature and number of moles affect the pressure of the gas particles (by selecting pressure with Rspd such that pressure cannot be controlled). Assume that 0.03 mol of helium at a temperature of 275.00 K occupy a volume of 1.40 L. Use the Run Experiment tool in the Simulation to determine the initial pressure of the gas and the new pressure values when the temperature or number of moles is changed to complete the following statements. Match the words in the left column to the appropriate blanks in the sentences on the right. Make certain each sentence is complete before submitting your answer. The initial pressure of the helium gas is 0.48 atm use ideal gas equation : PV = n RT from this equation we can calculate initial pressure. and it is 0.483 atm From the initial conditions (0.03 mol and 275.00K), if you increased the amount of helium to 0.07 mol, the new pressure would be 1.13 atm . Therefore, pressure increases from this equation. with the number of moles in direct proportion. P is increases with increases in moles and Temperature From the initial conditions (0.03 mol and 275.00K), if you increased the temperature by 80.00 K, the new pressure would be 0.28 atm . Therefore, pressure increases with temperature in direct proportion. V increases with increase in moles and temperature only pressure decreases with volume moles decreases with temperature.