QUESTION 1 Under conditions of constant temperature and volume, how many additional moles of gas would...
Under conditions of constant temperature and volume, how many additional moles of gas would have to be added to a flask containing 1.96 moles of gas at 25.0 C and 1.00 atm pressure in order to increase the pressure to 2.3 atm?
A sample of carbon monoxide gas occupies a volume of 263 mL at a pressure of 781.3 torr and a temperature of 399 K. What would its temperature be if the volume were changed to 82 mL at a pressure of 657.5 torr? QUESTION 2 Under conditions of constant temperature and volume, how many additional moles of gas would have to be added to a flask containing 2.7 moles of gas at 25.0 °C and 1.00 atm pressure in order...
Under constant-volume conditions, 3100 J of heat is added to 1.9 moles of an ideal gas. As a result, the temperature of the gas increases by 78.5 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc.
Under constant-volume conditions, 4100 J of heat is added to 1.5 moles of an ideal gas. As a result, the temperature of the gas increases by 132 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc.
Please help with these two 1. A flask is filled with 1.08 moles of a gas at 20.7 K and 646.8 mm Hg. The flask is then opened and an additional 1.33 moles are added. The temperature of the flask is then changed to 272.4 K. What is the pressure (in atm) of the flask under these final conditions? 2. The density of a gas is 4.22 g/L at a pressure of 1.77 atm and a temperature of 14.66 °C. What...
L. Under that conditions of temperature and pressure would you expect gases to obey the ideal-gas equation? 2 Calculate the value of R in L-atm/mol-K by assuming that an ideal gas occupies 3 Why do you equalize the water levels in the bottle and the beaker? 5 What is the value of an error analysis? 224 Lmol at STP 4 Why does the vapor pressure of water contribute to the total pressure in the bottle? Suggest reasons why real gases...
QUESTION 2 What amount (in moles) of a gas is contained in 40.4 L at-82.4 °C with a pressure of 527.4 mm Hg? QUESTION 3 A flask is filled with 1.03 moles of a gas at 13.4 K and 618.9 mm Hg. The flask is then opened and an additional 1.84 moles are added. The temperature of the flask is then changed to 172.9 K. What is the pressure (in atm) of the flask under these final conditions? QUESTION 4...
How many moles of neon are present in 44.8 L of neon under the conditions of standard temperature and pressure (273.0K; 1.00atm)? In this case, is it convenient to use the gas constant of 0.08206 L atm mol^-1K^-1?
QUESTION 3 0.5 points Save Answer A flask is filled with 1.56 moles of a gas at 14.2 K and 636.7 mm Hg. The flask is then opened and an additional 1.56 moles are added. The temperature of the flask is then changed to 136.3 K. What is the pressure (in atm) of the flask under these final conditions? QUESTION 4 0.5 points Save Answer What is the density in g/L) of a gas with a molar mass of 177.9...
help please Chapter 15, Problem 036 GO Under constant-volume conditions, 3000 J of heat is added to 1.3 moles of an ideal gas. As a result, the temperature of the gas increases by 185 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc. the tolerance is +/-2% Open Show Work Click if you would like to Show Work for this question: