Concept explainers
Interpretation:
The pressure setting used to obtain a
Concept Introduction:
The final pressure of the gas at the varying temperatures can be calculated using Gay-Lussac’s law, which states the relationship between pressure and temperature of the gas.
According to Gay-Lussac’s Law, for the gas held at constant volume, the pressure of a given amount of gas is directly proportional to the temperature of the gas. Mathematically, it is given as.
We two different sets of temperature and pressure of the gas is considered, the above equation becomes as follows:
where
Trending nowThis is a popular solution!
Chapter 5 Solutions
Introduction To General, Organic, And Biochemistry
- There are 1.07 X 10-3 moles of gas molecules contained in a CO2 cartridge under 5.0-atm of internal pressure. After several uses, the internal pressure is 3.4-atm. How many moles of gas remain in the cartridge? How much gas will remain in the cartridge when the internal pressure equilibrates to standard pressure? (Assume that the temperature and volume remain constant.)arrow_forward5. What was the starting pressure of a 8645 liter sample of butane at 14.00 degrees Celsius the volume changes to 9600 liters at STP 6. A 2.0 m^ 3 sample of propene was collected at STP. Find the new temperature of the propene if the new volume is 2.4m ^ 3 at pressure of 755 mm Hg.arrow_forward-Volume of trapped gas = 88.57 mL - moles of O2 = 0.00359- Pressure of trapped gas = 756 mmHg- Partial pressure collected O2 =732.2 mm Hg. - temperature = 298.15 Kd. From these results, calculate an experimental value for the ideal gas constant,R in L atm mol–1 K–1. e. Using 0.0821 as the true value for the gas constant, calculate the % error ofthe experiment to the nearest whole number.arrow_forward
- For many purposes we can treat ammonia (NH₂) a as an ideal gas at temperatures above its boiling point of -33. °C. Suppose the temperature of a sample of ammonia gas is lowered from 16.0 °C to -11.0 °C, and at the same time the pressure is changed. If the initial pressure was 0.46 kPa and the volume decreased by 55.0%, what is the final pressure? Round your answer to 2 significant digits. kPa 0.0 Xarrow_forwardA soda manufacturing company is experimenting with changing the taste of its product as the concentration of carbon dioxide changes. To track their results, they must determine how concentration changes with pressure. The concentration of CO2 under a partial pressure of 0.855 atm is 422.9 ppm. At what pressure (in atm) would the CO2 need to be so that the concentration of CO2 is 212.7 ppm at the same temperature? Report your answer to the thousandths place and do not include units.arrow_forward1. Where did the R constant in PV=nRT come from, and why must we convert everything to the units of the R constant? 2. Why does the density of water change with its temperature? 3. If all of the gas was not vaporized before taking the mass (some stayed in liquid form), how would that affect the final molar mass calculation? 4. If a sample of ethanol (C2H6O) was determined to have a pressure of 2 atm at a temperature of 25°C, what is its density (in g/L)?arrow_forward
- A 100-liter empty jar was spiked with 20 mg of TCE (C2HCl3) under room temperature condition. The jar was then closed tightly. What is the concentration (in atm.) of TCE in the air at 25 C? (TCE: MW: 131.4 g/mol; TCE solubility in water (Cs) = 1100 mg/L; Pv (pure liquid at 25oC) = 10^-1.01 atm. KH = 10^1.03 L atm mol-1; KOW = 102.42). if the jar was half filled with water and half filled with air, what were the concentrations of TCE in both air and water at 25C?arrow_forwardIn an offshore oil-drilling operation at 1500 m depth, gas X was found at the seabed at a temperature of 520 °C and pressure of 15.40 atm. i. Calculate the volume of gas X that needs to be transferred from the seabed to a valve container with a volume of 2.90 x 104 litres at the refinery tower if the pressure must be retained at 1.00 atm and the temperature at 21 °C. ii. Determine the mass of gas X that needs to be transferred. [Molar mass of X = 16 gmol-1]arrow_forwardHigh-pressure liquid chromatography (HPLC) is a method used in chemistry and biochemistry to purify chemical substances. The pressures used in this procedure range from around 500 kilopascals (500,000 Pa ) to about 60,000 kPa (60,000,000 Pa ). It is often convenient to know the pressure in torr. If an HPLC procedure is running at a pressure of 5.28×108 Pa , what is its running pressure in torr?arrow_forward
- High-pressure liquid chromatography (HPLC) is a method used in chemistry and biochemistry to purify chemical substances. The pressures used in this procedure range from around 500 kilopascals (500,000 Pa) to about 60,000 kPa (60,000,000 Pa). It is often convenient to know the pressure in torr. If an HPLC procedure is running at a pressure of 1.70×108 Pa, what is its running pressure in torr?Express the pressure numerically in torr.arrow_forwardIdeal Gas Law Fermentation of glucose produces gas in the form of carbon dioxide, how many moles of carbon dioxide are produced if 785 ml of carbon dioxide at 20.1°C and 90 kPa was collected during the process? where V = volume in liters P = pressure in atmosphere n = moles T=temperature in Kelvin R= universal gas constant, =0.0821 L atm/mol. K =8.314 L kPa/mol, Karrow_forward[a] The compound 1-iodododecane is a nonvolatile liquid with a density of 1.20g/mL. The density of mercury is 13.6g/mL. What do you predict for the height of a barometer column based on 1-iodododecane, when the atmospheric pressure is 749 ton? [b] What is the pressure, in atmospheres, on the body of a diver if he is 21 ft below the surface the water when the atmospheric pressure is 742 torr?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning