A 120. mL sample of a gas is at a pressure of 1.50 atm. If the temperature remains constant,
what will be its volume at 3.50 atm of pressure?
120 * 1.5/3.5 = 51.4 ml
To solve this problem, we can use the combined gas law, which relates the initial and final states of a gas sample.
The combined gas law is given by the formula: P1 * V1 / T1 = P2 * V2 / T2
In this case, we are given the following information:
- Initial volume (V1) = 120 mL
- Initial pressure (P1) = 1.50 atm
- Final pressure (P2) = 3.50 atm
- The temperature remains constant, so T1 = T2
We need to solve for the final volume (V2).
Rearranging the formula, we get: V2 = (P1 * V1 * T2) / (P2 * T1)
Since the temperature remains constant, T1 = T2. Therefore, we can simplify the equation to: V2 = (P1 * V1) / P2
Now, let's substitute the given values into the equation:
V2 = (1.50 atm * 120 mL) / 3.50 atm
Calculating the expression:
V2 = 51.43 mL (rounded to two decimal places)
Therefore, the volume of the gas at 3.50 atm of pressure would be approximately 51.43 mL.