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- a)A gas occupies an 8.00 mL flexible-walled container. The pressure is doubled, the absolute temperature is quadrupled, and 15% of the gas leaks out. What is the new volume? b) A sample of neon has a volume of 0.730 dm3 at a temperature of 21.0 °C. and pressure of 102.5 kPa. If the density of neon is 0.900 g/dm3 at 0 °C and 101.3 kPa, what is the mass of the sample? C) the radius of a copper bar is 4mm. What force is required to stretch the rod by 20% of its length assuming that the elastic limit is not exceeded? Y= 12×10^10N/m2 2. How much heat is needed to convert 1 kg of ice at -10℃ to steam at 100℃? Remember ice and water do not have the same specific heat.(a) A gas occupies an 8.00 mL flexible-walled container. The pressure is doubled, the absolute temperature is quadrupled, and 15% of the gas leaks out. What is the new volume? (b) A sample of neon has a volume of 0.730 dm3 at a temperature of 21.0 °C. and pressure of 102.5 kPa. If the density of neon is 0.900 g/dm3 at 0 °C and 101.3 kPa, what is the mass of the sample?A sealed container has a volume of 0.012 m3 and contains 26.5 g of molecular nitrogen (N2), which has a molecular mass of 28.0 u. The gas is at 157 °C. What is the absolute pressure of the nitrogen gas, in kilopascals? 1 u = 1.67 x 10-27 kg.
- 500 Ibm of methane gas is stored in a container of dimensions 4 m length, 4 m width and 6 m height under pressure of 200 kPa and temperature of 25 °C. What is the density of gas in the container in Kg/m'?Problem 6: Suppose a 26.5°C car tire contains 3.5 mol of gas in a 32.5 L volume. Part (a) What is the gauge pressure, in atmospheres, in the car tire? Pg1 = Part (b) What will the gauge pressure be if you add a quantity of gas that had a volume of 2.00L when it was at atmospheric pressure and the same temperature as the tire? Assume the temperature returns to 26.5°C and the volume remains constant.If an ideal gas has a pressure of 7.310 × 10° Pa, a temperature of 47.00 °C, and a volume of 0.0741 m³, how many moles n of gas are in the sample? n = mol
- If I have 2.9 L of gas at a pressure of 5.0 atm and a temperature of 50.°C, what will be the temperature of the gas if I decrease the volume of the gas to 2.4 L and change the pressure to 95.0 kPa?A large cylindrical tank contains 6.50 x10 cm of nitrogen gas at 28°C and 7.7 x10 Pa. a) The tank has a piston that allows the volume to be changed. What will be the pressure, in Pa, if the volume is decreased to 0.430 m and the temperature is increased to 155°C? b) If the temperature of the tank is kept constant at 28°C while the volume is decreased to 0.430 m, what would be the pressure of the tank in Pa? Express your answers to 1 d.p.How many moles of gas are in a bike tire with a volume of 2.00×10 – 3 m3(2.00 L), a pressure of 7.00×105 Pa (a gauge pressure of just under 90.0 lb/in2 ), and at a temperature of 18.0ºC ?
- Problem 6: Suppose a 26.5°C car tire contains 3.5 mol of gas in a 32.5 L volume. Part (a) What is the gauge pressure, in atmospheres, in the car tire? P21=1.65 vCorrect! Part (b) What will the gauge pressure be if you add a quantity of gas that had a volume of 2.00 L when it was at atmospheric pressure and the same temperature as the tire? Assume the temperature returns to 26.5°C and the volume remains constant. P22= 1.5| g,2Suppose a 26°C car tire contains 3.65 mol of gas in a 28.5 L volume. a)What is the gauge pressure, in atmospheres, in the car tire? b)What will the gauge pressure be if you add a quantity of gas that had a volume of 2.00 L when it was at atmospheric pressure and the same temperature as the tire?If I have 2.9 L of gas at a pressure of 5.0 atm and a temperature of 50.°C, what will be the temperature of the gas if I decrease the volume of the gas to 2.4 L and decrease the pressure to 25 psi?