gont get it.. To what temp must a sample of nitrogen at 27 degrees C and 0.625 atm be taken so that its pressure becomes 1.125 atm at constant volume

i used the formula and it still gave me a weird answer

That looks ok to me.

P1/T1 = P2/T2

T must be in Kelvin.

i still don't get it tho. is it 0.625*27/1.125?

Did you see my note about using Kelvin? The 27 is degrees C. It must be changed to KELVIN? Do you know how to do that? ALSO, you didn't multiply right (or you set up the equation wrong).

Make a table
Pressure Temperature
1.125........??
0.625........27 (change to Kelvin).
To solve you cross multiply the ratios.

oooh so 1.125 * 27/0.625

You have the multiplication down BUT you didn't change T of 27 C to KELVIN!

i don't know how to do that

Kelvin = 273.15 + C.

for this one i did

0.625....27+273= 300
1.125... T2
0.625=1.125
300= T2
1.125*300/0.625=540?

To solve this problem, we can use the ideal gas law equation, which states:

PV = nRT

Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature in Kelvin

In this case, the volume is constant, so the equation can be simplified to:

P1/T1 = P2/T2

Where:
P1 = Initial pressure
T1 = Initial temperature (in Kelvin)
P2 = Final pressure
T2 = Final temperature (in Kelvin)

Let's solve the problem step by step:

1. Convert the initial temperature from degrees Celsius to Kelvin. The Kelvin scale starts at absolute zero, so the temperature in Kelvin is obtained by adding 273.15 to the degrees Celsius temperature:

T1 = 27 + 273.15

2. Substitute the known values into the equation:

0.625 / T1 = 1.125 / T2

3. Rearrange the equation to solve for T2:

T2 = (T1 * P2) / P1

4. Substitute the known values into the equation:

T2 = (27 + 273.15) * 1.125 / 0.625

5. Calculate the final temperature, T2.

By following these steps, you should be able to obtain the correct answer for the final temperature.