CH 4 behaves more like an ideal gas than CCl 4. Explanation: The intermolecular interaction in CCl 4 is stronger than in the CH 4 molecule due to the presence of more electronegative chlorine atom in CCl 4. The gases with stronger intermolecular interaction deviate from ideal behaivour. At high temperature, gases behaves more like an ideal gas.

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Formula : μ rms = (3RT/M) ½ Where, R = Ideal gas constant => 8.3145 (kg m 2 /sec 2)/K mol T = Absolute temperature in Kelvin M = Molecular weight of the gas in kilograms Jan 30, 2018 · 58. In the ideal gas equation PV=nRT, the value of gas constant depend only on: a) The pressure of the gas b) The volume of the gas. c) The nature of the gas d) the units of measurement. 59. What is the normality of NH4OH solution having density of 0.6g/ml containing 34% by weight of. a) 0.1N b) 0.4N. c) 4.2N d) 5.8N. 3. 60.

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Calculate the pressure that ccl4 will exert at 40 of 1.00 mol occupies 28.0 L, assuming that (a) CCl4 obeys the ideal-gas equation (b) CCl4 obeys the Van der Waals equation. (a) PV = nRT

CCl4 is a non polar organic solvent. so for any comparible volume of solvents, CCl4 would hold more acid than water. Mar 28, 2012 · Determine the empirical formula of an oxide of iron which has 69.9% iron and 30.1% dioxygen by mass. Apr 18, 2020 · An ideal gas is a gas whose pressure P, volume V, and temperature T are related by the ideal gas law: PV = nRT. where n is the number of moles of the gas and R is the ideal gas constant. Ideal gases are defined as having molecules of negligible size with an average molar kinetic energy dependent only on temperature. Jun 13, 2010 · will be a gas at this pressure. The given pressure, 101.3 kPa is one atmosphere. So we can find the molar volume of it from the ideal gas formula, PV = nRT where. P is the pressure (1.0 atm.) V is the volume which we seek, n is the number of moles. of gaseous CCl4, R is the molar gas constant, 0.082054 liter-atm. per mole per °K,