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A sample of gas was labeled 15.20 kPa. How should this pressure be written in atmospheres ATM?
To convert kPa to atm, divide the pressure in kPa by 101.3 (since 1 atm = 101.3 kPa). Therefore, 15.20 kPa is equivalent to 0.150 atm when rounded to three decimal places.
A quantity of a gas has an absolute pressure of 400kPa and an absolute temperature of 110 degrees kelvinwhen the temperature of the gas is raised to 235degrees kelvin what is the pressure of the gas?
Using the combined gas law (P1/T1 = P2/T2), we can calculate the pressure of the gas at the new temperature. Plugging in the values, we get P2 = (P1 * T2) / T1 = (400 kPa * 235 K) / 110 K = 853 kPa. Therefore, the pressure of the gas is 853 kPa when the temperature is raised to 235 degrees Kelvin.
A helium-filled balloon contains 0.26 mol He at 101 kPa and a temperature of 21 and degC. What is the volume of the gas in the balloon?
To find the volume of the gas in the balloon, you can use the ideal gas law: PV = nRT. First, convert the temperature to Kelvin (21°C + 273 = 294 K). Then plug in the values: (101 kPa) * V = (0.26 mol) * (8.31 LkPa/(molK)) * (294 K). Solve for V to find the volume of the gas in the balloon.
What is the temperature of 0.80 mol of a gas stored in a 275 mL cylinder at 175 kPa?
To find the temperature, you can use the ideal gas law formula: PV = nRT. First, convert the volume to liters (275 mL = 0.275 L). Then plug in the values of pressure (175 kPa), volume (0.275 L), and number of moles (0.80 mol), and the gas constant (R = 8.314 J/mol*K) to solve for temperature (T).
Convert a pressure of 23.8 in Hg to kPa?
Pressure of 23.8 in Hg to kPa is equivalent to 80596.0582 Pa (pascal)
What is the pressure of gas in the flask in kPa if the barometer read 769.3 mmHg?
1 kiloPascal is equal to 7.5006 mmHg. So, using that conversion rate, it can be found that 769.3 mmHg is equal to 102.6 kPa.
How do you convert 345 kpa to barg?
To convert kilopascals (kPa) to bar gauge (barg), subtract the atmospheric pressure (typically around 101.3 kPa) from the given pressure. In this case, 345 kPa - 101.3 kPa = 243.7 kPa absolute. Then, convert the absolute pressure to barg by dividing by 100, as 1 bar = 100 kPa. Therefore, 243.7 kPa / 100 = 2.437 barg.
A sample of gas was labeled 15.20 kPa. How should this pressure be written in atmospheres ATM?
To convert kPa to atm, divide the pressure in kPa by 101.3 (since 1 atm = 101.3 kPa). Therefore, 15.20 kPa is equivalent to 0.150 atm when rounded to three decimal places.
A quantity of a gas has an absolute pressure of 400kPa and an absolute temperature of 110 degrees kelvinwhen the temperature of the gas is raised to 235degrees kelvin what is the pressure of the gas?
Using the combined gas law (P1/T1 = P2/T2), we can calculate the pressure of the gas at the new temperature. Plugging in the values, we get P2 = (P1 * T2) / T1 = (400 kPa * 235 K) / 110 K = 853 kPa. Therefore, the pressure of the gas is 853 kPa when the temperature is raised to 235 degrees Kelvin.
What is 47.3 kPa converted into degrees Celsius?
Pressure cannot be directly converted into temperature as they are different units of measurement. Pressure is typically measured in pascals (Pa) or kilopascals (kPa) whereas temperature is measured in degrees Celsius (°C). To convert pressure to temperature, you would need additional information such as the volume and the ideal gas law.
How kPa convert to mm Hg?
Conversion for kPa to mmHG: kPa x 7.501 = mmHg202.6 kPa x 7.501 = about 1,520 mmHg
A helium-filled balloon contains 0.26 mol He at 101 kPa and a temperature of 21 and degC. What is the volume of the gas in the balloon?
To find the volume of the gas in the balloon, you can use the ideal gas law: PV = nRT. First, convert the temperature to Kelvin (21°C + 273 = 294 K). Then plug in the values: (101 kPa) * V = (0.26 mol) * (8.31 LkPa/(molK)) * (294 K). Solve for V to find the volume of the gas in the balloon.
How do you convert 1780 kpa to ATM?
When using the pressure formula. PV=nRT. Pressure(in ATM) x Volume(in liters)=n(number of moles) x R(gas constant=.0821) x Temperature(in kelvins)If you are given pressure in kpa you have to convert to ATM
What is the temperature of 0.80 mol of a gas stored in a 275 mL cylinder at 175 kPa?
To find the temperature, you can use the ideal gas law formula: PV = nRT. First, convert the volume to liters (275 mL = 0.275 L). Then plug in the values of pressure (175 kPa), volume (0.275 L), and number of moles (0.80 mol), and the gas constant (R = 8.314 J/mol*K) to solve for temperature (T).
How do you convert 2.5 ATM to kpa?
ATM x 101.325 = kPa So, 2.5 x 101.325 = 253.312 kPa
What is the ideal gas contact?
The ideal gas constant has different values depending on the units one uses for pressure. Thus, if using atmospheres, R = 0.0821 L-atm/K-mole. If using kPa, R = 8.314 L-kPa/K-mole, and if using mm Hg, R = 62.36 L-mm Hg/K-mole.
A gas sample occupies 4.2 L at a pressure of 101 kPa. What volume will it occupy if the pressure is increased to 235 kPa?
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
