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What is the temp of 4 moles of gas at a pressure of 8.3 mmHg and a volume of 163 mL in K?
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What are the four variables in the ideal gas law?
Pressure, volume, temperature & the amount of gas.
If you have mL degrees Celsius and mmHg figure out Volume at STP?
That's going to depend on the substance, which the question neglects to identify. --------------------------------------------------- The volume of any gas at STP (pressure of 1 ATM & temp.: 0oC) is approximately 22.41 L/mol or 22,410 mL/mol. So you need to find out how much gas you have to begin with (# of moles) to find the volume of the gas at STP.
What is the name of the scientific law air pressure and volume?
The scientific law that relates air pressure and volume is Boyle's law. It states that at a constant temperature, the pressure exerted by a gas is inversely proportional to its volume. In other words, as the volume of a gas decreases, its pressure increases, and vice versa.
Under which conditions will the volume of a given sample of a gas always decrease?
The Ideal Gas Law states that PV=nRT, where P=pressure, V=volume, n=number of moles of gas, R=the relativity constant, and T=temp in Kelvin. According to this law, volume (V) varies as V=(nRT)/P. Using this, we can determine that the volume would normally increase with an increase in the number of moles and/or an increase in the temperature and/or a decrease in pressure. Therefore, we can logically determine that the volume of a gas would decrease in the instance of increasing temperature if either the number of moles of gas was decreased or the pressure was increased (to an extent where the level of volume increase by temperature change has been overcome.)
What is the pressure of 3.80 moles of oxygen be at a temp of 299 K and a volume of 11.3 L?
This equation is applicable: pV=nRTp = 3,8 x 0,082057 x 299/11,3 = 8,25 atmospheres
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.).
What volume will ml of gas at 20 degree celsius and a pressure of 355 mm hg occupy if the temperature is reduced to 80 degree celsius and pressure increased to 760 mm hg?
Let's see if I have the question correct?Initial volume = 1 mLInitial Temp = 20 oC ie 293 KInitial Pressure = 355 mmHg or 47.3 kPaFinal values -Final volume = ? or unknownFinal Temp = 80 oC ie 353KFinal Pressure = 760 mmHg or 101.3 kPaAssuming the gas is acting as an ideal gas. That is the gas has no extra attraction to other molecules of the gas in the sample.The Gas Law states thatP1V1/T1 = P2V2/T2355 x 1 /293 = 760 x ? /80V2 = 9.5 mL
How many moles of gas does a steel cylinder witha volume of 45 liters contain at standard temp pressure?
stp= 22.4 dm3, 1L = 1 dm3 1mole ---> 22.4dm3 xmole ---> 45dm3 45/22.4 = 2.001 moles
What happens to pressure when the temperature and volume is halved?
if kelvin temp is halved, the volume is halved if pressure is constant.
What is the relationship between the kelvin temperature and the pressure of gas?
Increased temperature = increased volume of gas The above answer is non-sense. The pressure could increase with temperature and actually yield a smaller volume... here ya go: The ideal gas law is: PV = nRT, where P = pressure, V = volume, n= number of moles, R = ideal gas constant, T = Temperature in K
How to calculate final pressure when given initial pressure and initial temp and also final temp and know that it's a constant volume process from initial state?
You can calculate pressure and temperature for a constant volume process using the combined gas law.
What 2 things can make the pressure of gas rise?
1) Increase in heat 2)Decrease in volume
