# Question #a651a

##### 1 Answer

#### Explanation:

Notice that no mention was made about the *number of moles of gas* and the *volume* of the cylinder, which means that you can ssume them to be **constant**.

In this case, you know that pressur eand temperature have a **direct relationship** when the number of moles of gas and the volume of the container are kept constant - this is known as Gay Lussac's Law.

In other words, if the temperature *increases*, the pressure *increases* as well. If the temperature *decreases*, the pressure *decreases* as well.

In your case, the pressure of the sample of gas **decreased** from

This means that the temperature of the sample **decreased** as well,so you can expect the temperature on th previous day to be a little *higher* than

Mathematically, Gay Lussac's Law can be written like this

#(P_1)/T_1 = P_2/T_2" "# , where

Plug in your values and solve for

#T_1 = P_1/P_2 * T_2#

#T_1 = (4.88color(red)(cancel(color(black)("atm"))))/(4.69color(red)(cancel(color(black)("atm")))) * 8^@"C" = 8.324^@"C"#

I'll leave the answer rounded to two sig figs, despite the fact that you only gave one sig fig for the temperature of the gas

#T_1 = color(green)(8.3^@"C")#