For an ideal gas , PV=nRT
Or,V=nRT/P
Where,R=universal gas constant=0.0821 L atm K-1 mol-1)
T=temperature
(standard temp=273K)
P=pressure (std P=1 atm)
N= number of moles
V1=n1RT/P=(1.00 mol)* RT/P
V2=n2RT/P=(2.00 mol)* RT/P
V1/V2=1/2
2V1=V2
Putting the values of P,R.T,
V1=n1RT/P=(1.00 mol)*(0.0821 L atm K-1 mol-1)*(273K)/1 atm=22.413L
V2=2*V1=2*22.41L=44.82 6L
V2=44.826L
Imagine that the gas shown in the simulation is an ideal gas such as helium. Notice...
If the volume of a certain gas is changed from V_1 to V_2, the corresponding change in number of moles will be from n_1 to n_2. For such a case, Avogadro's law can also be expressed as V_1/n_1 = V_2/n_2 where n_1 and n_2 are the initial and final numbers of moles of the gas and V_1, and V_2 are the initial and final volumes of the gas, respectively. In an ideal gas, particles are considered to interact only when...
V_1 (100 cc) cubic centimetres of helium, assumed to be an ideal gas, at P_1 = 10 atm, in contact with a reservoir at T_1 = 10 degree K, is to be expanded to 1 atm. by allowing part of the gas to enter a volume V_2 in contact with a reservoir at T_2 = 290 degree K. How large is V_2? What is the ratio of the masses of gas in the volumes V_1 & V_2?
Imagine 1.00 mol of helium (ideal) gas in a variable-volume system initially at 0.82 atm and 236 K. The pressure is fixed, and the temperature is increased to 341 K. Calculate q (J) for this system.
A 2.60-mol sample of helium gas initially at 300 K, and 0.400 atm is compressed isothermally to 1.00 atm. Note that the helium behaves as an ideal gas. (a) Find the final volume of the gas. (b) Find the work done on the gas. (c) Find the energy transferred by heat.
A 2.60-mol sample of helium gas initially at 300 K, and 0.400 atm is compressed isothermally to 1.00 atm. Note that the helium behaves as an ideal gas. (a) Find the final volume of the gas.? m3 (b) Find the work done on the gas. kJ (c) Find the energy transferred by heat. kJ
Let us first examine the behavior of an ideal gas when we force the volume to be a value of our choosing. We can examine how changes to the absolute temperature and number of moles affect the pressure of the gas particles (by selecting pressure with Rspd such that pressure cannot be controlled). Assume that 0.03 mol of helium at a temperature of 275.00 K occupy a volume of 1.40 L. Use the Run Experiment tool in the Simulation to...
EXAMPLE 6-11 Applying the Ideal Gas Equation to a Mixture of Gases What is the pressure, in bar, exerted by a mixture of 1.0 g H2 and 5.00 g He when the mixture is confined to a volume of 5.0 L at 20 °C? Analyze For fixed T and V, the total pressure of a mixture of gases is determined by the total number of moles of gas: Ptot = ntotRT/V. Solve ntot = (1.0g Hz x 1 mol Hy)...
10...11
P_1V_1/T_1 = P_2V_2/T_2 PV = nRT M = mRT/PV R = 0.08206 L middot atm/mol middot K A teaching assistant was determining the molar volume of nitrogen gas, N_2(g). (MW: 28.0131 g/mol). at standard temperature and pressure. The TA found that 146 mL of gas was collected at 21.0 degree C and 0.968 atm. The TA determined the volume of this gas sample at STP (1.00 atm and 273 K) is ____ mL. Your answer should be expressed with...
A 1.60-mol sample of helium gas initially at 300 K, and 0.400 atm is compressed isothermally to 1.40 atm. Note that the helium behaves as an ideal gas. (a) Find the final volume of the gas. (b) Find the work done on the gas. (c) Find the energy transferred by heat.
Assume that helium behaves as an ideal monatomic gas. If 76 moles of helium undergo a temperature increase of 245 K at constant pressure, how much energy (in J) has been transferred to the helium as heat? Round your answer to the nearest whole number.