----------The temperature of a constant amount of an ideal gas in a closed system ata fixed pressure, p₁, was increased while the volume was measured. Thisexperiment was repeated twice more at pressures p2 and p3 and theresults from all three experiments are shown in the graph below.P3P₁TIdentify the CORRECT relationship between these three pressures.a. p1>P2 P3b. p₁ = P2 P3C. p1 P2 P3Oe. p₁ > P2 = P3Rank the following four substances in order of increasing boiling point.O a. H₂ C4H10 A reaction in a container releases 120 kJ of heat to the surroundings and 50kJ of work is done on the system by the surroundings. Calculate the changeof internal energy, AU, of the system.O a. AU = +70 kJO b. AU=-70 kJC. AU = 0 kJ (no change).O d. AU +170 kJO e. AU = -170 kJA 10 g metal bar is heated to 498 K immediately before it is immersed into abeaker containing 100 mL of water which has an initial measuredtemperature of 298 K (the beaker is surrounded by polystyrene to minimizeany loss of heat). After immersion of the hot bar, the temperature of thewater increases to 320 K. A diagram of this experiment is shown below:Calculate the amount of heat that is transferred from the bar into the water.(density of water = 1.00 g mL and specific heat capacity of water = 4.18 JK-1g-1).O a. +9.20 kJO b. +4.18 kJO c. –9.20 kJO d. +0.920 kJO e. -0.920 kJ

Since you have asked multiple questions, we will solve the first question for you. If you want any…

The temperature of a constant amount of an ideal gas in a closed system at a fixed pressure, p₁, was increased while the volume was measured. This experiment was repeated twice more at pressures p2 and p3 and the results from all three experiments are shown in the graph below. P₁ P₁ T Identify the CORRECT relationship between these three pressures. Ⓒap₁>P2P2 P3 Oep₁>P2=P3 P₂

The temperature of a constant amount of an ideal gas in a closed system at a fixed pressure, p₁, was increased while the volume was measured. This experiment was repeated twice more at pressures p2 and p3 and the results from all three experiments are shown in the graph below. P₁ P₁ T Identify the CORRECT relationship between these three pressures. Ⓒap₁>P2P2 P3 Oep₁>P2=P3 P₂

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

the answer of part A is 0.721
Underwater, the pressure increases by 1 bar for every 10 m of depth. When a scuba diver breathes pressurized air in which the partial pressure of N2(g) exceeds 4 bar, the result is nitrogen narcosis, which is similar to alcohol intoxication. What is the maximum mole percent of N2 in an air mixture that could be used by divers at depths up to 85 m below sea level without undue risk of nitrogen narcosis?
The pressure of a sample of neon gas at 171.2°C and 75.4 kPa was increased to 91.1 kPa. What is the new temperature of the neon gas in °C?
When air expands adiabatically (without gaining or losing heat), its pressure P and volume V are related by the equation PV14 = C where C is a constant. Suppose that at a certain instant the volume is 310 cubic centimeters and the pressure is 87 kPa and is decreasing at a rate of 8 kPa/minute. At what rate in cubic centimeters per minute is the volume increasing at this instant? cm3 min (Pa stands for Pascal it is equivalent to one Newton/(meter squared); kPa is a kiloPascal or 1000 Pascals.
A canister of pressurized gas has a mass of 10.0000 g. A small amount of gas is released and collected. The collected gas has a volume of 50.00 mL. The pressure and the temperature of the collected gas are the same as the air pressure and air temperature that day: 100. kPa and 25oC. It is noticed that when the gas is released the mass of the pressurized canister decreases to a mass of 9.9110 g. It is not known what gas is in the canister, but you know it is one of the following gases: methane (CH4), ethane (C2H6), propane (C3H8) or butane (C4H10). Using the information provided determine which gas is actually present in the canister.
p+a |(V-nb)=nRT The van der Waals equation of state. R stands for the gas constant and n for moles of gas. The parameters a and b must be determined for each gas from experimental data. Use the van der Waals equation to answer the questions in the table below. х10 What are the units of a? What are the units of b? For ethane the numerical value of a is 5.507 and the numerical value of b is 0.0651. ||atm Use the van der Waals equation to calculate the pressure of a sample of ethane at 90.0 °C with a molar volume of 8.59 L/mol. Round your answer to 3 significant digits. Use the Ideal Gas Law to calculate the pressure of the same sample under the same conditions. Round this answer to 3 significant digits also. atm