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Identify the law that is associated with this formula PV c?
The formula PV = C is done by the Gas Law to measure pressure and volume's relationship.
How many moles of carbon dioxide are there in 800 cm3 of gas at 30 C and 110 kPa?
0.035mol. Apply to PV=nRT
What is the mass of CO2 gas inside a 7.949 L glass bulb at a pressure of 2.906 x 10-1 ATM at 52 degrees C?
Use the Ideal Gas law ... PV = nRT n = number of moles. Temp must be kelvin not celsius. R is the ideal gas constant so ... n = PV/(RT) Substitute in appropriately and get an answer for # of moles. CO2 has a molar mass of 44 multiply moles by 44 to find mass in grams.
A 150.0 ML sample of gas is collected at 1.20 ATM and 25 C what volume does the gas have at 1.50 ATM and 20.0 Ccould you show work?
PV/T=PV/T 1.20 ATM * 150.0 ML / 25 C = 1.50 ATM * V / 20.0 C 1.20 ATM * 150.0 ML / 298 K = 1.50 ATM * V / 293.2 K 1.20 ATM * 150.0 ML / 298 K / 1.50 ATM * 293.2 K = V 118 ML = V
What volume would be occupied by 0.50 moles of gas at a temperature of 35 degrees C and a pressure of 1ATM?
pV=ntR V= (.5)(35+273)(8.314)/1 =approx. 1280.4
Identify the law that is associated with this formula PV c?
The formula PV = C is done by the Gas Law to measure pressure and volume's relationship.
What law is associated with PV equals c?
Boyle's Law
What law matches this formulaPV c?
Boyle's Law, but it does go further than PV = c.
What law is this PV c?
It may be Boyle's law, but there is not enough context in the question to be sure.
What is the volume of helium gas that 5.10 moles occupies at 10 C and 0.95 ATM?
From the combined gas law, PV = nRT, solve for V.V = nRT/P = (5.10)(0.082)(283)/0.95 = 125 liters
What is the temperature of 0.57mol of gas at a pressure of 1.5atm and a volume of 11.4L?
Using the Ideal Gas Law pV=nRT, I can solve for T by isolating for it giving me T=pV/nR. n=0.57 mol, p=1.5 atm=151.875 kPa, R= gas constant= 8.314 kPaL/molK, and V=11.4 L. Calculating for T, I get an answer of 365.4... K. Changing that into Celsius which is Kelvin-273.15 and I get 92.197...°C. Round it to two significant digits and I get 92°C.
Which of the following is an expression of Boyle's law A equals constant B PT equals constant C equals constant D PV equals constant?
C.
How many moles of carbon dioxide are there in 800 cm3 of gas at 30 C and 110 kPa?
0.035mol. Apply to PV=nRT
What volume will 400ml of argon gas initially at 30degree celsius and 725mmHg occupy at 30 degree celsius and 650mmHg?
PV/T = PV/T ( forgot who's law that is ) need to convert C to K 30 C = 303.15 K (725 mmHg)(400 ml)/(303.15 K) = (650 mmHg)(X Vol)/(303.15 K) 197047.5X = 87913500 = 446 ml ---------------
What amount (moles) of carbon dioxide gas is present in a compressed cylinder (900 mL) at 300 kPa at 25.0 C?
Using ideal gas law...in metric units, thanks. 786 torr = 104658 Pa 900 mL = 0.0009 m3 22 C = 295.15 K R = 8.314 J/K-mol PV = nRT n = PV / RT = 104658 x 0.0009 / 8.314 x 295.15 = 0.0384 mol
What is the mass of CO2 gas inside a 7.949 L glass bulb at a pressure of 2.906 x 10-1 ATM at 52 degrees C?
Use the Ideal Gas law ... PV = nRT n = number of moles. Temp must be kelvin not celsius. R is the ideal gas constant so ... n = PV/(RT) Substitute in appropriately and get an answer for # of moles. CO2 has a molar mass of 44 multiply moles by 44 to find mass in grams.
A 325-mL sample of air is at 810.5 torr and 30.0 C What volume mL will this gas occupy at 900.0 torr and 60.0 C?
I got 321.6mL. You use PV=nRT to find n, and plug that into PV=nRT with the new conditions to find the new volume.
