What is the temperature of an 11.2 l sample of carbon monoxide, co, at 744 torr if it occupies 13.3l at 55 degrees celsius and 744 torr?

Taking into account the Charles's law,  the temperature of an 11.2 L sample of carbon monoxide, CO, at 744 torr is 276 K or 3 C.

First of all, you have to know that Charles's Law consists of the relationship that exists between the volume and the temperature of a certain quantity of ideal gas.

This law says that when the amount of gas and pressure are kept constant, the quotient between the volume and the temperature will always have the same value:

Studying two different states, an initial state 1 and a final state 2, it is satisfied:

In this case, you can apply Charles's law because it can be seen that the pressure is constant, with a value of 744 torr at the beginning and end of the analysis. Then, you know:

Replacing in Charles's law:

Solving:

T₁= 276 K= 3 C

Finally, the temperature of an 11.2 L sample of carbon monoxide, CO, at 744 torr is 276 K or 3 C.

Learn more:

3 °C

Explanation:

The pressure is constant, so this looks like a case where we can use Charles’ Law:

Invert both sides of the equation.

Multiply both sides by V₂

V₁ = 13.3 L; T₁ = (55 + 273.15) K = 328.15 K

V₂ = 11.2 L; T₂ = ?

nacl is added to the aqueous of what? ? in order to get a proper answer you have to specify the exact composition of the aqueous solution.

c is the answer because when something is left after something evaporates that shows the chemical change.