Convert 13.0 atm to torr. 13.0 atm = 9880 Torr Convert 836 mmHg to atmospheres. 836 mmHg = 1.1 atm Convert 760 Torr to millimeters of mercury. 1 760 Torr = mmHg Incorrect

Q: Convert the following 34.5 atm= mmHg 30.39 kPa= torr

A: We have given that 34.5atm =                mmHg 30.39kPa =                 torr

Q: A flask stoppered to a volume of 125. mL is heated from 18.56 °C to 6b.00 °C. If the intial pressure…

A: Gay-Lussac's law: The relation between pressure and temperature at constant valume was found by…

Q: [References] Consider the flasks in the following diagram. 2.00 L H2 1.00 L N2 455 torr 0.220 atm…

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Q: 87 J0 T UOnsand Convert 836 Torr to atmospheres. 836 Torr = atm - TOOLS x10 Convert 13.0 13.0 atm =…

A: 1) 836torr to atm  We know that, 1atm = 760torr  Then,  = 836torr × ( 1atm / 760torr )  = [ 836 /…

Q: Convert pressures into atmospheres 48.2 kPa 1250 torr 75.5 torr

A: The following units of pressure are to be converted into atmospheres-  a)  48.2 kPa  b)  1250 torr…

Q: -5 atm to kPa 50 atm to bar -937 kPa to torr

A: Answer 1)    76cm Hg is equal to                 =  1 atm  then ,  76.8cm Hg is equal to = (76.8 ×…

Q: A gas occupies 12.3 liters at a pressure of 40.0 mmHg. What is the volume when the pressure is…

A: We will use the Boyle's law of ideal gas equation to calculate the final volume of the gas =>…

Q: Convert 13.0 atm to torr. 13.0 atm = - TOOLS Convert 836 x10' 836 mmHg = Convert 760 Torr to…

A: Answer : a)  760 torr = 1 atm  So , 836 torr = 1× 836/760            = 1.1 atm  b) 1 atm= 760 torr…

Q: A mixture of 7.0 grams of nitrogen gas and 48.0 grams of helium has a pressure of 12.0 atm under…

A: we have to calculate the partial pressure of nitrogen

Q: torr to atmospheres

A: Torr and atmosphere bhot are the units to measure the pressure  We are provided with pressure in…

Q: 28.5 inches of Hg. Convert this value to atmospheres

A: 1 inch of Hg = 0.0334 atm

Q: Convert 533 torr to atmospheres.

A: We know that,     1 atm=760 torr So, 1 torr=1/760 atm

Q: A gas sample with a constant number of gas molecules and at a constant temperature has a volume of…

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Q: 10.00 L of a gas is at 100 atm. What pressure is obtained when the volume is 10.0 L? 100 Kpa 100 atm…

A: Given :  Initial volume = 10.00 L Initial pressure = 100 atm Final volume = 10.0 L Final pressure =…

Q: A student reads a barometer in the laboratory and finds the prevailing atmospheric pressure to be…

A: The relation between different units of pressure is as follows: 1 atm=760 mm Hg1 atm=760 torr1…

Q: The atmospheric pressure on top of Mt. Everest (elevation 29,028 ft) is 0.329 atm. Calculate the…

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Q: Convert each pressure unit to the indicated unit. Remember to use the correct number of significant…

A:

Q: 14.6

A: Given State-1 V1= 80.3 L P1 = 1460 torr T1 = 35oC State-2 V2= ? P2 = 2480 torr T2 = 35oC

Q: 13.2 g of CO2 is mixed with 3.20 g of CH4 in a 4.00 L flask at a temperature of 11.2°C. What is the…

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Q: convert 680 torr to mmHg

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Q: onvert 0.997 atm to mmHg.      mmHg   b) Convert 648 torr to bar.      bar   c) Convert 628 kPa to…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Convert a pressure of 1800.0 torr to atm.

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Q: A sample of gas is stored in an manometer, and the mercury column is 61 mmHg lower on the side open…

A: atm and mm Hg are units to measure pressure. Both are related as 1atm = 760 mm Hg.

Q: The partial pressure of nitrogen in the atmosphere is 593. mmHg. Calculate the partial pressure in…

A: The objective of this question is to convert the given partial pressure of nitrogen from millimeters…

Q: A sample of 3.50 moles of helium gas at 25 degree Celsius exert a pressure of 505 torr. When more…

A: A sample of 3.50 moles of helium gas at 25 degree Celsius exert a pressure of 505 torr. When more…

Q: 921 torr to atm   340. kPa to atm    750. mmHg to kPa

A: Conversion of pressure measurements--

Q: Convert 836 Torr to atmospheres. 836 Torr = atm Convert 10.5 atm to torr. 10.5 atm = Torr Convert…

A: Pressure is force exerted per unit area. It can be expressed in a number of different units like…

Q: Which pressure is equal to 1.943 atm? A) 1477 torr B) 2.557 x 10-3 mmHg C) 391.1 torr D) 1302 mmHg

A: Unit conversion is applicable to convert the standard units from their one form to anotherwithout…

Q: The partial pressure of argon in the atmosphere is 7.10 mmHg. Calculate the partial pressure in atm…

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Q: Suppose that the volume of a particular sample of chlorine gas 8.170 L at 891.0 torr and 23.60…

A: Option (3) is correct. [ 2.03e+00 ]

Q: A closed flask containing nitrogen gas at 745 torr and 154 K is heated to 308 K. What is the new…

A: Gay-Lussac's law- As pressure increases, temperature increases at constant volume Given by equation-…

Q: A sample of a gas occupies 160.0 mL at -10.0?C and 620. torr. What pressure will the gas exert in a…

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Q: A 32.8 L balloon is filled with 78.0 grams of CO2 at 14.5 0C, what is the pressure of the balloon…

A: By assuming the ideal behavior of CO2 and knowing the molar mass of CO2, we can calculate the…

Q: sample of gas occupies a volume of 579 mL at 0.785 atm and 37 oC. Calculate the pressure of the gas…

A: V1 = 579 mL = 0.579 L P1 = 0.785 atm T1 = 37° C =( 37 + 273) K = 310 K = T2 V2 = 521 mL = 0.521 L…

Q: A 2.00-L glass soda bottle filled only with air is tightly capped at 34°C and 744.0 mmHg. If the…

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Q: A sample of gas has a volume of 2.4 L and a pressure of 1.2 atm. What would the pressure of the same…

A: Boyle’ law states that at a particular temperature the pressure of a gas is inversely proportional…

Q: 105.0 mL sample of gas was compressed to 15.0 mL where its pressure is 250.0 torr. What was the…

A: Given that the no. of moles is constant and the temperature at which the compression is done remains…

Q: A 0.75 mole sample of helium gas initially at 37.0°C, 785 torr and 9.45 L was heated to 58.0°C while…

A:

Q: A 10.00-L tank contains helium gas at 2.5 atm. What is the pressure of the gas in mmHg? O 304 mmHg O…

A: Volume(V) = 10.00 LPressure(P) = 2.5 atmPressure in mmHg =?

Q: Convert the following pressures into atmospheres.1. 105.2 k 2. 752 mm Hg

A: The objective of this question is to convert the given pressures from kilopascals (kPa) and…

Q: if 2.0 g of oxygen gas and 4.0 g of nitrogen gas are placed in a sealed 1.0 L container at 298K,…

A: According to ideal gas law, PV = nRT where P = total pressure V = volume of container n = total…

Q: A gas mixture contais each of the following gases at the indicated partial pressure. N2 - 219 torr…

A: The objective of the question is to find the total pressure of a gas mixture. The total pressure of…

Q: Determine the density of Ne(g) at 834 torr and 414 °C. 0.299 g/L 0.652 g/L 0.393 g/L 0.428 g/L…

A: Given, Pressure, P = 834 torr = (834/760) atm Temperature, T = 414 oC = (273.15 + 414) K = 687.15 K…

Q: A 3.0 L container of neon gas has a pressure of 1.0 atm. What will the pressure be if the volume is…

A: The objective of this question is to find the new pressure of the neon gas when the volume is…

Q: Convert 836 Torr to atmospheres. 836 Torr = atm Convert 20.0 atm to torr. 20.0 atm = Torr Convert…

A: GIVEN  Change in pressure  units like atm, torr ,mmofHg

Q: Convert 208 kPa into both atmospheres and torr. Select one: O a. 3060 torr, 4.02 atm O b. 0.274 atm,…

A: Interpretation: We have to convert 208 KPa to atm and torr.

Kinetic-Theory of Gases

Kinetic theory of gases is the model or method which was developed in the 19th century by Maxwell and Boltzmann. This is possible as the interatomic force which is of short-range forces that are important for solids and liquids can be neglected for gases. This theory or gas law gives a molecular interpretation of the pressure and temperature of a gas and is consistent with gas laws and Avogadro’s hypothesis. This theory is very helpful to correctly explain the specific heat capacities of many gases, kinetic energy and it also explains the transport qualities such as viscosity, thermal conductivity, and diffusion with molecular parameters. As stated in the kinetic-molecular theory, the temperature of a substance or gas particle is related to the average kinetic energy of the particles of that substance. When a substance is heated, some of the absorbed energy is stored within the particles, while some of the energy increases the motion of the particles, called average kinetic energy.