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When 4.38 g of calcium nitrate are heated strongly at 550 oc and 100 kPa, complete decomposition occurs as shown. 2CaO(s) + 4N02(g) + 02(g) Calculate the volume, in m3 of the gaseous products. Give your answer to three significant figures. The gas constant is R = 831 J K-1 mol-I [5 marks]
How many moles of gas (air) are in the lungs of an adult with a lung capacity of 3.9 L? Assume that the lungs are at 1.00 atm pressure and at a body temperature of 40 oC. ∙ % (Hint: V, P, and T are given. Use the equation PV = nRT where R = 0.082058 ) ∙.
What is the molecular weight of this gas? Solution: This problem, as well as the two just above can be solved with PV = nRT. You would solve for n, the number of moles. Then you would divide the grams given by the mole calculated. 1) Use PV = nRT: (1.00 atm) (19.2 L) = (n) (0.08206) (273 K) n = 0.8570518 mol (I'll keep a few guard digits)
The Ideal Gas Law. PV = nRT. P = Pressure (in kPa) V = Volume (in L) T = Temperature (in K) n = moles. R = 8.31 kPa • L. K • mol. R is constant. If we are given three of P, V, n, or T, we can solve for the unknown value. Recall, From Boyle’s Law: P1V1 = P2V2 or PV = constant From combined gas law: P1V1/T1 = P2V2/T2 or PV/T = constant. Ideal Gases.
The Ideal and Combined Gas Laws PV = nRT or P1V1 = P2V2. T1 T2. Use your knowledge of the ideal and combined gas laws to solve the following problems. If it involves moles or grams, it must be PV = nRT. 1) If four moles of a gas at a pressure of 5.4 atmospheres have a volume of 120 liters, what is the temperature? 1973 K.
29 lip 2024 · This ideal gas law calculator will help you establish the properties of an ideal gas subject to pressure, temperature, or volume changes. Read on to learn about the characteristics of an ideal gas, how to use the ideal gas law equation, and the definition of the ideal gas constant.
Mass = number of moles x RFM. Mass = 0.0404 x 69.6. =2.81 g. also watch out if they give you the moles of a solid in the question. You can’t use this in PV = nRT, you have to use the ratio → moles of gas.
