# Question #a317c

##### 1 Answer

#### Explanation:

The idea here is that when the volume of the gas and the number of moles of gas present in your sample remain *constant*, **increasing** the temperature of the gas will cause its pressure to **increase** as well **Gay Lussac's Law** here.

Mathematically, this can be written like this

#color(blue)(ul(color(black)(P_1/T_1 = P_2/T_2)))#

Here

#P_1# ,#T_1# are the pressure and absolute temperature of the gas at an initial state#P_2# and#T_2# are the pressure and absolute temperature of the gas at final state

In your case, the temperature of the gas is **increasing**, so you should expect to find

#P_2 > "0.96 atm"#

Rearrange the equation to solve for

#P_1/T_1 = P_2/T_2 implies P_2 = T_2/T_1 * P_1#

Plug in your values to find

#P_2 = (684 color(red)(cancel(color(black)("K"))))/(478color(red)(cancel(color(black)("K")))) * "0.96 atm" = color(darkgreen)(ul(color(black)("1.4 atm")))#

The answer is rounded to two **sig figs**, the number of sig figs you have for the initial pressure of the gas.