7. a gas occupies 4.31 liters at a pressure of 0.785 atm. determine the volume if the pressure is increased…

7. a gas occupies 4.31 liters at a pressure of 0.785 atm. determine the volume if the pressure is increased to 1.25 atm.\n8. a sample of gas at 3.00 mm hg inside a steel tank is cooled from 500.0 °c to 0.00 °c. what is the final pressure of the gas in the steel tank?\n9. if i have 15 moles (numbers) of gas held at a pressure of 560 atm, how many moles of gas do i have if i increase pressure to 764 atm?\n10. a weather balloon contains 8.80 moles of helium at a temperature of 25 °c at ground level. what is the new temperature if i add 1.2 moles to the balloon under these conditions?\n11. if a gas in an expandable container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original moles was 1.55, how many moles would there be after the container is pressurized?\n12. a 12.00 - liter box had 4.50 moles of chlorine gas. if 2.00 moles of chlorine gas entered the box, what is the new volume of the box, assuming pressure and temperature stayed constant.

7. a gas occupies 4.31 liters at a pressure of 0.785 atm. determine the volume if the pressure is increased to 1.25 atm.\n8. a sample of gas at 3.00 mm hg inside a steel tank is cooled from 500.0 °c to 0.00 °c. what is the final pressure of the gas in the steel tank?\n9. if i have 15 moles (numbers) of gas held at a pressure of 560 atm, how many moles of gas do i have if i increase pressure to 764 atm?\n10. a weather balloon contains 8.80 moles of helium at a temperature of 25 °c at ground level. what is the new temperature if i add 1.2 moles to the balloon under these conditions?\n11. if a gas in an expandable container is pressurized from 15.0 atmospheres to 16.0 atmospheres and its original moles was 1.55, how many moles would there be after the container is pressurized?\n12. a 12.00 - liter box had 4.50 moles of chlorine gas. if 2.00 moles of chlorine gas entered the box, what is the new volume of the box, assuming pressure and temperature stayed constant.

Answer

Explanation:

Step1: Identify initial and final states

Initial moles $n_1 = 4.50$ moles, initial volume $V_1=12.00$ L, moles added $\Delta n = 2.00$ moles. So final moles $n_2=n_1+\Delta n=4.50 + 2.00=6.50$ moles.

Step2: Apply Avogadro's law

Since pressure and temperature are constant, Avogadro's law states $\frac{n_1}{V_1}=\frac{n_2[SSE Completed, Client Connection Error][SSE Completed, Client Connection Error][LLM SSE On Failure]