When you punch the numbers into your calculator, however, make sure you use the stored values you got from the actual conversions, and not the rounded ones. All we need to do is divide this by volume, and we have density: How do we find density? Notice we're given the mass of the sample (0.622 g). Convert 574.5 mmHg to atm, torr, Pa, and kPa. So, we have almost everything we need to simply plug into the equation. 757.75 MPa (megapascal) 7726.89960384 kgf/cm2 (kg per sq. View Notes - chem1211 hw 10 from CHEM 1211 at University Of Georgia. Just something to take note of.Д«ack to the problem: Now, looking back at what we're given, we will need to make some unit conversions to ensure everything matches the dimensions required by the equation: R = Ideal Gas Constant ( #~~0.0821 (atm*L)/(mol*K)#)ДЄs an aside, note that because calculations with this equation involve molar mass, this is the only variation of the ideal gas law in which the identity of the gas plays a role in your calculations. Hence, just take my word for it that you will end up with the equation: The derivation is simple but for the sake of time and space, I will skip it. 25.299743133 atm (standard atmosphere) 26.140389154 at (technical atmosphere) 19227.804781439 torr 261403.92966075 mmH2O (mm of water) 19227.804781439 mmHg (mm of mercury) 757 inHg (inches of mercury) 371.804122412 psi (pounds per sq. Here is a repeat from the 'Four Variables' file:There are three different units of pressure used in chemistry.

To solve this, however, we will first need to play with the combined ideal gas equation #PV = nRT# to make it work for density and molar mass. PSI can be expressed using the formula: 1 psi 1 lbf in 2. What is the pressure of the gas in the mercury manometer, It is useful to remember that 760 mmHg1.000 atm101.3 kPa The pressure of a gas in a container is often measured relative to atmospheric pressure using a manometer.This is a U-shaped tube containing mercury and connecting the container to the air (Figure 2). Rearrange the Ideal Gas Law to this: V nRT / P Substitute values into the equation: V (3.00 mol) (0.08206 L atm molВЇ1 KВЇ1) (297.0 K) / (762.4 mmHg / 760. Calculate the volume 3.00 moles of a gas will occupy at 24.0 вЊ and 762.4 mm Hg. Whenever you see molar masses in gas law questions, more often than not density will be involved. Multiply the answer (which is in atm) by 760.0 mmHg atmВЇ1 to get mmHg.

757 mmhg to atm