Login or Sign Up

Ask a New Question

The gas in a large balloon has a volume of 1.35 liters and a pressure of 1.75 atm. What will the pressure be if the volume is increased to 3.15 liters?

Please show work.

AAAaannndd the bot gets it wrong yet again!

right numbers, yet still gets the wrong answer!

3.15P = 1.35 * 1.75
P = 0.75 atm

The pressure of a gas is inversely proportional to its volume, so the pressure will decrease when the volume increases. We can use the equation P1V1 = P2V2 to calculate the new pressure.

P1V1 = P2V2
1.75 atm x 1.35 L = P2 x 3.15 L
P2 = 0.848 atm

Similar Questions

A mickey mouse balloon has a maximum volume of 10.0 liters. A little boy purchased a MM balloon at Disneyland. It has a pressure

Top answer: See your previous post. It's (P1V1/T1) = (P2V2/T2) Substitute and see the value of V2 and if that Read more.
Select the correct answer.A pressure of 2 kilopascals (Pa) is acting on a gas with a volume of 60 liters. If the pressure

Top answer: P1V1 = P2V2 Substitute the numbers and solve for V2 Post your work if you get stuck Read more.
A large balloon contains 65.0 L of helium gas at 25 °C and a pressure of 745 mm Hg. The balloon ascends to 3000 m, at which the

Top answer: If the temperature remains constant, then Boyles law applies: PV=constant Here P1=745 mmHg V1=65 L Read more.
A balloon contains 0.113 mol of gas and has a volume of 3.06 L. If an additional 0.178 mol of gas is added to the balloon (at

Top answer: To find the final volume of the balloon after adding 0.178 mol of gas, we can use the principle of Read more.
I have a balloon that contains 22 grams of Carbon dioxide. The barometric pressure is 1019 millibars which I converted to 1.006

Top answer: To determine the correct volume of the balloon using the ideal gas law, we need to utilize the Read more.
I have a balloon that contains 22 grams of Carbon dioxide. The barometric pressure is 1019 millibars which I converted to 1.006

Top answer: Remember at STP one mole is 22.4 liters, you have one half mole, at near STP. Your answer is Read more.
Assume that the balloon is filled with carbon dioxide gas at 20°C and standard pressure. Use the ideal gas law to calculate the

Top answer: Why did the balloon go to the party? Because it wanted to have a gas-tly good time! Now, to Read more.
A sample of gas in a balloon has an initial temperature of 28 and a volume of 1360 . If the temperature changes to 86, and there

Top answer: 28 WHAT? 1360 WHAT? Use (V1/T1) = (V2/T2) Don't forget T1 and T2 must be in kelvin. Read more.
A balloon contains 3.3 liters of nitrogen gas at a temperature of 90K and a pressure of 101 kPa.If the temperature of the gas is

Top answer: since PV/T is constant, if P is held constant, then V/T is constant. if T is increased by a factor Read more.
The volume of air in a balloon is 4.5 liters when inflated. External pressure decreases the volume to 1.1 liters. If the

Top answer: equation looks good ... Boyle's Law Read more.

Did you know?

Did you know that the pressure of a gas is inversely proportional to its volume, assuming temperature remains constant? This means that as the volume of a gas increases, the pressure decreases, and vice versa. In this scenario, if the volume of a gas in a large balloon is initially 1.35 liters and has a pressure of 1.75 atm, and then the volume is increased to 3.15 liters, we can calculate the new pressure. By using the equation P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume, we can solve for P2. Plugging in the given values, we get 1.75 atm * 1.35 L = P2 * 3.15 L. Simplifying this equation, we find that P2 is approximately 0.749 atm. Therefore, when the volume increases to 3.15 liters, the pressure will decrease to 0.749 atm.