A volumetric pyrex flask is calibrated at 20 ° C. The flask is filled, up to the 100 mL mark, with acetone at 35 ° C. (a) What is the volume of the acetone cooled to 20 ° C? Where β = 1.5 x 10-4 ° C-1 of the ketone. (b) How significant is the change in the volume of the bottle?
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A volumetric pyrex flask is calibrated at 20 ° C. The flask is filled, up to the 100 mL mark, with acetone at 35 ° C. (a) What is the volume of the acetone cooled to 20 ° C? Where β = 1.5 x 10-4 ° C-1 of the
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- A 10.0 L container contains a certain gas at a temperature of 25.0◦C and pressure of 9.50 atm. Calculate the number of moles of gas in the container.A young male adult takes in about 5.87 x 10-4 m3 of fresh air during a normal breath. Fresh air contains approximately 21% oxygen. Assuming that the pressure in the lungs is 1.09 x 105 Pa and air is an ideal gas at a temperature of 310 K, find the number of oxygen molecules in a normal breath.A room is 10.0 m by 7.5 m by 2.7 m is filled with air at 22oC and 1 atm. The average molar mass of air is 28.8 g/mol. Find the number of moles of air to fill the room and the weight of the air in kg.
- On a hot summer day, the density of air at atmospheric pressure at 35 °C is 1.1455 kg/m3. What is the number of moles contained in 1 m3 of ideal gas at this temperature and pressure? Avogadro’s number of air molecules has a mass of 2.85×10-2kg. what is the mass of 1 m3 of air? Does the value calculated in part (B) agree with the stated density of air at this temperature?In a sealed bottle, the temperature is raised from 200k to 400k. What happens to the remaining quantities? Pressure (P): (doubles / halves / stays constant ) Volume (V): (doubles / halves / stays constant ) Moles (n): (doubles / halves / stays constant ) Gas constant (R): (doubles / halves / stays constant ) Temperature (T): (doubles / halves / stays constant )If the dew point of air (35°C and 1 atm) is 20 °C, what is the RH under that temperature and pressure (35°C and 1 atm)? What is the volume fraction?
- Three moles of an ideal gas at 135C and 0.5 atm is allowed to expand 1 atm at a constant pressure to a volume twice as large. What is the new temperature?Problem 3. The viral coefficients of a gas at 20 °C and 11.5 bar are B = -138 cm³ mol¹ and C=7222 cmº mol². Calculate the V (molar volume) Z (compressibility factor) of the gas. Use the equation below (R = 83.14 cm³ bar mol-¹ K-¹). PV 2 = ² = (1 + = + =) Z RT