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What volume is occupied by 2.0g He at 25 degrees celsius and 775 mmHg?
Wiki User
∙ 6y ago
A fixed quantity of gas at a constant pressure exhibits a temperature of 27 degrees Celsius and occupies a volume of 10.0 L. Use Charles's law to calculate:
the temperature of the gas in degrees Celsius in atmospheres if the volume is increased to 16.0 LWiki User
∙ 6y ago
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What is the temperature in degree celsius of a 2.75 L of gas at 47 degrees celsius and 798 mmHg?
47 degrees Celsius
751.5 mmHg is how many atmospheres?
751.5 mmHg = 0.9888 atmospheres
How many atmosphere are there in 1000 mmHg using 1 atm is equal to 760 mmHg is 760 torr?
The answer is in the question itself:760 mmHg (= 760/760 ) = 1.00 atm , so1000 mmHg = 1000/760 = 1.32 atm
Angelo noticed his lab partner had incorrectly recorded the pressure of a gas in mmHg rather than in atmospheres as their teacher requested When he corrected the mistake Angelo recorded 751.5 mmHg?
the answer is 0.99 :)
What is the formula for AA gradient?
PAO2 - PaO2 ****************************************** PAO2 is the Alveolar Air Equation: PAO2 = FiO2 (Pb- Ph20) - PACO2/R Notes: Pb = 760 mmHg Ph20 = 47 mmHg R = 0.8
What volume will 400 ml of argon gas initially at 30 degree celsius and 725 mmHg occupy at 30 degree celsius and 650 mmhg?
The volume is 0,446 L.
Will measured a gas at 30 degrees Celsius and 752.0 mmHg what would his measurements be if expressed in kelvin and atmospheres?
30 degrees Celsius = 303,15 K752 mmHg = 0,9894737 atmosphere
What is the temperature in degree celsius of a 2.75 L of gas at 47 degrees celsius and 798 mmHg?
47 degrees Celsius
How do you convert celsius to mmhg?
To convert temperature from Celsius to mmHg, you would need to convert the Celsius value to Kelvin first. Then, you would use the formula pv = nRT, where p is the pressure in mmHg, v is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin to calculate the pressure.
What is the volume in milliliters occupied by 89.2g CO2(g) at 37oC and 737 mmHg?
To find the volume of a gas using the ideal gas law formula PV = nRT, we need to know the molar mass of CO2 (44.01 g/mol) and convert grams to moles. Then we can rearrange the formula to solve for V (volume) using P (pressure), n (moles), R (gas constant), and T (temperature). After plugging in the values (P = 737 mmHg, T = 37°C + 273 = 310 K), we can calculate the volume occupied by 89.2g of CO2 gas.
What is the vapour pressure of water at 65 degrees?
The vapor pressure of water at 65 degrees Celsius is approximately 170.4 mmHg.
How do you convert degrees Celsius per mm Hg to just degrees Celsius?
You can't. Celsius per mmHg is a relationship of temperature to pressure. You can however solve for temperature if you have the value of pressure (e.g. if P= 10 mmHg and V/P = 2 ºC/mmHgthen V= (2 ºC/mmHg)(10 mmHg) = 20 ºC). If you have more information in the problem you might be referring to Gay-Lussac's Law, which compares two values of pressure and temperature to show the relationship (GL'sL: P1/T1 = P2/T2 ... but that would be pressure per unit volume). I'm not sure what you are looking for exactly, but you can't convert temp. to pressure (just like you can't convert feet to lbs.).
Does STP stand for zero degrees celsius and 760 mmHg?
No, STP stands for Standard Temperature and Pressure, which is defined as 0 degrees Celsius and 1 atmosphere (101.3 kPa) pressure. 760 mmHg is equivalent to 1 atmosphere pressure.
What is the expression for the ideal gas law?
PV=nRT (pressure*volume=mols*value for R*temperature in degrees kelvin) R Values vary, but must match the unit for pressure---> .0821 ATM 62.4 mmHg 8.314kPa temperature must always be in degrees kelvin ( kelvin= degrees celsius+273)
According the reference table h what is the vapor pressure of propanone at 45 degrees Celsius?
The vapor pressure of propanone (acetone) at 45 degrees Celsius is approximately 365 mmHg according to reference table h.
If you have mL degrees Celsius and mmHg figure out Volume at STP?
To convert mL at a certain temperature to volume at STP (standard temperature and pressure of 0 degrees Celsius and 1 atm pressure), you would need to apply the ideal gas law equation PV = nRT. First, convert mL to L, then use the temperature to find the new volume. If you have the pressure in mmHg, you'll also need to convert that to atm.
Vapor pressure of ethylene glycol at 25 degree celsius?
757.2 mmHg is almost atmospheric pressure (P = 760 mmHg) and therefore the vapour pressure is very close to the normal boiling point.According to the boiling temperature is T = 353.14 K = 79.99 °C at P = 757.2 mmHg.
