Calculate the temperature of 4.00 moles of ideal gas at a pressure of 2.00 atm and a volume of 54.0 L. (Use 0.0821 L · atm/mol · K as the gas constant.)

- Determine what happens to the pressure of the above sample of ideal gas if the volume is halved and the temperature doubles.

A student states that if the volume of a sample of ideal gas increases to three times the original volume, and the pressure also increases to three times the original pressure, the temperature of the gas will remain unchanged.

- Explain why the student is incorrect.
- Determine the actual temperature of the ideal gas.

answer; natural resources;

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.