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The ideal gas law measures pressure in?
The ideal gas law measures pressure in pascals (Pa) or atmospheres (atm).
If the ideal gas constant has a value of 0.0821 what are its units?
L •atm/mole•k
How do you get ATM to molarity?
The "Ehow" website containing an excellent article on determining the ATM to molarity. It is, however, a most complex process and requires a barometer, extra long tape measure and a thermometer.
A sample of a gas pressure of 3.00atm at 25c what would the gas pressure be at 52c if the volume remaiins constant?
25C is 298K. 52C is 325K. Assuming linearity (an ideal gas), P=3*325/298=3.27 atm.
What best describes the molecules of an ideal gas?
Molecules of an ideal gas are considered to be point masses that do not have any volume, do not interact with each other, and collide with each other and the container walls in perfectly elastic collisions. The behavior of ideal gases is described by the ideal gas law, which relates pressure, volume, and temperature.
The ideal gas law measures pressure in?
The ideal gas law measures pressure in pascals (Pa) or atmospheres (atm).
If the ideal gas constant has a value of 0.0821 what are its units?
L •atm/mole•k
If the ideal gas constant has a value of 0.0821 what are the units?
L •atm/mole•k
If 43.5 moles of an ideal gas is at 4.59 ATM at 50.40 and degC what is the volume of the gas?
The volume is 251,6 litres.
If the ideal gas constant has a value of 0.0821 what are it's units?
L •atm/mole•k
How can the ideal gas law be simplified to Avogodro's Law?
If a sample of an ideal gas has a volume of 2.22 at 287 K and 1.13 atm what will the pressure be when the volume is 1.47 L and the temperature is 306 K?
What is the relationship between internal energy and the behavior of an ideal gas?
The internal energy of an ideal gas is directly related to its temperature. As the temperature of an ideal gas increases, its internal energy also increases. This relationship is described by the equation for the internal energy of an ideal gas, which is proportional to the temperature of the gas.
How do you get ATM to molarity?
The "Ehow" website containing an excellent article on determining the ATM to molarity. It is, however, a most complex process and requires a barometer, extra long tape measure and a thermometer.
A sample of a gas pressure of 3.00atm at 25c what would the gas pressure be at 52c if the volume remaiins constant?
25C is 298K. 52C is 325K. Assuming linearity (an ideal gas), P=3*325/298=3.27 atm.
What best describes the molecules of an ideal gas?
Molecules of an ideal gas are considered to be point masses that do not have any volume, do not interact with each other, and collide with each other and the container walls in perfectly elastic collisions. The behavior of ideal gases is described by the ideal gas law, which relates pressure, volume, and temperature.
The gas pressure in an aerosol can is 1.8 ATM at 25oC If the gas is an ideal gas what pressure would develop in the can if it were heated to 475oC?
Using the ideal gas law (PV = nRT), we can calculate the new pressure of the gas in the aerosol can. Given that the initial pressure (P1) is 1.8 ATM and the initial temperature (T1) is 25°C, we can rearrange the formula to find the new pressure (P2) at 475°C. Since the volume (V), moles of gas (n), and gas constant (R) remain constant, we can solve for P2: P2 = (P1 * T2) / T1 = (1.8 ATM * 748 K) / 298 K ≈ 4.5 ATM.
What is volume occupied by a mole of an ideal gas if the pressure is 626mmHg and the temperature is 25.0C?
The volume occupied by a mole of an ideal gas can be calculated using the ideal gas law equation: PV = nRT. Convert the pressure to atm (1 atm = 760 mmHg), and the temperature to Kelvin (25.0°C = 298 K). Then substitute the values into the equation and solve for volume (V).
