The pressure of gaseous Al 2 Cl 6 increases more rapidly with temperature than predicted by the ideal gas equation even though Al 2 Cl 6 behaves like an ideal gas has to be explained. Concept introduction: First, we have to understand the concept of pressure of gas and their relationship with temperature. According to ideal gas law , the approximation of behavior of so many gases under some conditions and which is also called as general gas equation. The ideal gas equation represented as P V = n R T . Where, P represents pressure of gas, V represents volume of gas, n represents amount of gas substance, R represents universal gas constant, and T represents absolute temperature of gas. From ideal gas equation, we can say that pressure is directly proportional to temperature.

Question

Want to see the full answer?

Answer 1

Question

Chapter 21, Problem 21.55QP

Interpretation Introduction

Interpretation:

The pressure of gaseous Al2Cl6 increases more rapidly with temperature than predicted by the ideal gas equation even though Al2Cl6 behaves like an ideal gas has to be explained.

Concept introduction:

First, we have to understand the concept of pressure of gas and their relationship with temperature.

According to ideal gas law, the approximation of behavior of so many gases under some conditions and which is also called as general gas equation.

The ideal gas equation represented as PV=nRT .

Where, P represents pressure of gas, V represents volume of gas, n represents amount of gas substance, R represents universal gas constant, and T represents absolute temperature of gas.

From ideal gas equation, we can say that pressure is directly proportional to temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

A metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and temperature of the cylinder when it was initially filled were 120 atm and 75 ◦C, respectively. The molar mass of carbon is 12 g·mol−1 and the molar mass of hydrogen is 1 g·mol−1. a) How many moles of propane are in the cylinder? b) What is the mass of the propane inside the cylinder? c) After some time, the cylinder and its contents cool to 25 ◦C. What is the pressure in the cylinder after it has cooled?

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based on experimentally collected data, the student calculates R to equal L'atm 0.0832 mol·K L'atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error =|1.389 (b) For the statements below, identify the possible source(s) of error for this student's trial. The student uses the barometric pressure for the lab to calculate R. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student does not clean the zinc metal with sand paper. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it.