# A tank holds 2.36 l of gas at 784 torr and 24.2 C. How much will it occupy at STP(standard temp. and pressure?

This problem would involve the ideal gas law: PV=nRT. By algebra, we can rearrange as this: PV/T=nR. Since neither n or R ever change, we can equate the two states. Thus, P1V1/T1=P2V2/T2.

Now, let's get all of our data and put it into good units.
P1 = 784 torr = 1.03 atm
V1 = 2.36 L
T1 = 24.2 C = 297.2 K

P2 = 1 atm
V2 = ?
T2 = 273.15 K

Now, we insert and solve.

((1.03)*(2.36)) / 297.2 = ((1)*(V2)) / 273.15

V2 = 2.234 L = 2,234.095 mL
aaply the formula yourself:

P1V1/T1 = P2V2/T2

Standard Temperature = 20 C
Standard Atmosphere = 760 torr

Therefore T2 would be 273+20 degrees Kelvin, in absolute units.

The answers post by the user, for information only, FunQA.com does not guarantee the right.

More Questions and Answers:
• How many milliliters of a 25% (m/v) NaOH solution would contain 75 g of NaOH?
• Does phosphoric acid react violently when combined with copper sulphate?
• How to solve this?( a chemistry question)?
• How to verify a the heat capacity of a coffee-cup calorimeter?
• How could you separate a mixture of gravel and sand?
• Calculating molarity?
• What is 2 x 3?
• Is a Copper (II) Ion mean it is Cu2+ or Cu2-? or neither?
• What is a good household agent that will neutralize acid in the soil?