Question: The relationship between temperature and volume of a gas is linear and given by Charl's law V (ml) = Constant × T (°C) T(°C) -23 -13 -3 7 17 27 37 47 57 67 77 V (ml) 8.41525 8.75186 9.08847 9.42508 9.76169 10.09830 10.43491 10.77152 11.10813 11.44474 11.78135 Calculate the temperature (°C) at which the volume of the gas become close to zero.
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- Scottish physicist W. J. M. Rankine proposed an absolute temperature scale based on the Fahrenheit degree, now called degree Rankine abbreviated R and used by some engineering fields. If a degree Rankine is 5/9 of a degree Kelvin, what is the value of the ideal gas law constant in L. atm/mol. R?Pressure Volume 18 kPa 60.0 ml 21 kPa 50.0 ml 27 kPa 40.0 ml 35 kPa 30.0 ml 54 kPa 20.0 ml 104 kPa 10.0 ml 212 kPa 5.0 ml An alternative method of determining an equation for Boyle's Law is to graph the inverse of either the pressure or the volume. Calculate the inverse of the pressure and plot that versus the volume for the set of data above. What is the equation of the best fit line in the form: 1/P=aV+b The value of a is Question 7 options: A) 9.3x104 B) 9.3x10-4 C) 1.79x10-4 D) 1.79x104Calculate the pressure exerted in atm by 3.0 moles of ammonia when it is behaving as (a) a perfect gas in atm at 25°C in 22.414L and (b) van der Waals (VDW) gas at 100°C in 1000.0 cm3. Given van der Waals constants: a(NH3) (L2.atm/mol2) = 4.17 and b(NH3)(L/mol) = 0.037. The pperfect gas = .............atm and pVDW = ................ atm 3 sig. figures normal format.
- An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air).Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2. V2 = VM =A 500.0 mL sealed canister only containing exactly 0.1209 mol of methylamine (CH3NH2) is heated to 330.0 °C.All of the methylamine will have vapourized.Use Van der Waal's equation to calculate the pressure.(Pobs+[(n2a)/(V2)])(V−nb)=nRTFor methylamine: a=7.13 L2 atm/mol2; b=0.05992 L/mol.An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air). Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2. Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2. A) V2 = Now, suppose that the above experiment generated n mol of H2(g), that T2 = 0 °C and that P2 = 1 atm. Give the simple algebraic expression, in terms of V2 and n, which equates to the molar volume of H2(g) at STP. B) VM =
- An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air).Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2.Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2. V2 = Now, suppose that the above experiment generated n mol of H2(g), that T2 = 0 °C and that P2 = 1 atm. Give the simple algebraic expression, in terms of V2 and n, which equates to the molar volume of H2(g) at STP.VM = 8.829×10-4 mol of B2H6(g) (diborane gas) is generated into a 176.0 mL headspace, at 25.0 °C, thus increasing the pressure by 0.1209 atm. If we assume that the diborane gas obeys Boyle's Law and Charle's Law, what…An experiment is conducted in which a quantity of H2(g) is chemically generated in a closed headspace of volume V1 at absolute temperature T1, thereby raising the total pressure from Pa (the initial air pressure) to Pf (the total final pressure of H2(g) + air).Compose an algebraic expression for the volume (V2) that this sample of H2(g) would occupy if it were isolated (pure -- i.e. no air) at absolute temperature T2 and partial pressure P2.Note that your expression may contain no other variables than those given above, namely: V1, T1, T2, Pa, Pf, and P2.Calculate the pressure exerted in atm by 3.0 moles of ammonia when it is behaving as (a) a perfect gas in atm at 25°C in 22.414L and (b) van der Waals (VDW) gas at 100°C in 1000.0 cm3. Given van der Waals constants: a(NH3) (L2.atm/mol2) = 4.17 and b(NH3)(L/mol) = 0.037. Use 273.15 K for the temperature conversion. Pperfect gas = [A] atm PVDW = [B] atm 3 sig. figures normal format. Note: There is no need to add the units. The numerical values is sufficient as long as it is calculated in atm. Please also indicate the sign if it is necessary without a space from the numerical answer.
- A sample of H2 gas is collected over water at 21.5 degrees C and atmospheric pressure is 765 torr. The height of liquid in the eudiometer is 13.0 cm. What is the partial pressure of the H2 gas? Make sure to convert cm to mm and use density ratio. Use equation: PH2 = Pbarometric - PH2O - Pliquid column.....................An 85 g-mol gas 0ccupies 38 L at 78oC,,, wh@t is the vacuum pressure 0f the gas in psi??? CH0iceS: 210.4421 195.7421 -195.742 225.1421 961.6895 946.9895 932.2895 -932.289The pressure on 900 mL of a gas is 130 kPa. What must the pressure be changed to in order to make the volume 0.600L? (please show work)