P1; 83 kPa
Standard Pressure (P2); 101.3kPa
T1= 35 C
= 308.15 K (Kelvin)
P1/T1 = P2/T2
83 kPa/308.15 K = 308.15 K/T2
0.269 = 308.15 K/T2
T2 = 308.15/0.269
T2= 1145.53903 K
Gay-Lussac's Law: Ti T Don't forget to convert 'C to K obni 1. 9.0L of a...
o. Pi P2 Gay-Lussac's Law: Ti T2 Don't forget to convert °C to K 1. 9.0 L of a gas is exerts a pressure of 83.0 kPa at 35.0°C. What would be the required temperature (in °Celsius) to change the pressure to standard pressure?
T1 T2 Gay-Lussac's Law: Don't forget to convert 'C to K 1. 9.0L of a gas is exerts a pressure of 83.0 kPa at 35.0°C. What would be the required temperature (in ℃elsius) to change the pressure to standard pressure? 4
According to Amontons’s law or Gay-Lussac's law, which states that the pressure of a gas is proportional to the temperature of the gas, what would be the pressure of a gas at absolute zero? Select the correct answer below: 0 1 atm ∞ depends on the gas
Gay-Lussac's law states that the pressure of a gas is directly related to its absolute temperature, provided the volume and number of moles of the gas remain the same: (Figure 1) Part A A sample of ideal gas is in a sealed container. The pressure of the gas is 145 torr, and the temperature is 39 °C. If the temperature changes to 80 °C with no change in volume or amount of gas, what is the new pressure, P2, of the gas...
Perform calculations using Gay-Lussac's Law Question A gas in a sealed container has an initial pressure of 125 kPa at 25.0°C. If the pressure is increased to 150.0 kPa, what will the new temperature be? • Report your answer with three significant figures. • Use -273.15°C for absolute zero. Provide your answer below:
1.Gay-Lussac's Law A gas container is initially at 47 mm Hg and 77 K (liquid nitrogen temperature.) What will the pressure be when the container warms up to room temperature of 25 ˚C? 2. A container of gas is initially at 0.500 atm and 25 ˚C. What will the pressure be at 125 ˚C? 3.A toy balloon has an internal pressure of 1.05 atm and a volume of 5.0 L. If the temperature where the balloon is released is 200...
Perform calculations using Gay-Lussac's Law Question A gas in a sealed container has an initial pressure of 125 kPa at 25.0° C. If the pressure is increased to 150.0 kPa, what will the new temperature be? Report your answer with three significant figures. Use -273.15°C for absolute zero. Provide your answer below: degrees Celsius FEEDBACK MORE INSTRUCTION SUBMIT Content attribution
from gay-lussac's law, If you increase the temperature of a gas (with constant moles and volume) what do you expect will happen to the pressure? Look up Boyle's Law. For an ideal gas at constant temperature and moles, if you increase the volume of the gas what do you expect will happen to the pressure of the gas? How else is the pressure-volume relationship typically plotted?
4. a) Define Gay-Lussac's law. b) In equation form, Gay-Lussae's law is 5. A Chem 1314 student determines the mass of an unknown gas to be 0.99 grams at 43 °C and 745 mm Hg in a 200 mL container. What is the molecular mass of the unknown gas? [show work] The "unknown" gas (among the following) is most probably a) propane, CH. b) sulfur hexafluoride, SF6c) Xenon, Xe d) pentane, CHia CHEM1314-YEAR 2019-2020
The ideal gas law (PV=nRT) describes the relationship among pressure P, volume V, temperature T, and molar amount n. Fix n and V When n and V are fixed, the equation can be rearranged to take the following form where k is a constant: PT=nRV=k or (PT)initial=(PT)final This demonstrates that for a container of gas held at constant volume, the pressure and temperature are directly proportional.The relationship is also called Gay-Lussac's law after the French chemist Joseph-Louis Gay-Lussac, one of...