1. A balloon at 0.98 atm contains 0.16 mol of CH4, 0.23 mol of N2, 0.012...
7. A balloon at 0.98 atm contains 0.16 mol of CH4, 0.23 mol of N2, 0.012 mol of He and 0.018 mol of H2. What are the partial pressure of each gas? 8. A gas in a 2.00 L of ballon weigh 7.14 g at 2.00 atm and 27.0°C. What is the molar mass of the gas? 9. Sulfuric acid (H2SO.), the industrial chemical produced in greatest quantity (almost 45 million tons per year in the United States alone), is...
7. A balloon at 0.98 atm contains 0.16 mol of CH4, 0.23 mol of N2, 0.012 mol of He and 0.018 mol of H2. What are the partial pressure of each gas? 8. A gas in a 2.00 L of ballon weigh 7.14 g at 2.00 atm and 27.0 C. What is the molar mass of the gas? 9. Sulfuric acid (H2SO4), the industrial chemical produced in greatest quantity (almost 45 million tons per year in the United States alone),...
A gas mixture contains 0.600 mol of N2, 0.150 mol of H2, and 0.400 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 8.00 L vessel at 27.00°C. A) What is the total pressure in the vessel (atm)? B) What is the pressure (atm) of H2? C) What is the pressure (atm) of N2? D) What is the pressure (atm) of CH4?
A gas mixture contains 0.650 mol of N2, 0.200 mol of H2, and 0.200 mol of CH4. Calculate the pressure of the gas mixture and the partial pressure of each constituent gas if the mixture is in a 14.0 L vessel at 27.00°C. v 4th attempt Part 1 (1 pt) X Feedback See Periodic Table D See Hint total pressure in the vessel $ 2.70 atm Part 2 (1 pt) *Feedback pressure of H2 0.560 atm Part 3 (1 pt)...
Question-5 (2 marks) The total pressure of three gases in a balloon is 4.5 atm. The balloon contains 2.0 moles of O2, 3.0 moles of N2 and 5.0 moles of H2. What is the partial pressure of N2 gas in the balloon?
Suppose that Daniel has a 2.50 L bottle that contains a mixture of O2, N2, and CO2 under a total pressure of 4.70 atm. He knows that the mixture contains 0.23 mol N2 and that the partial pressure of CO2 is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O2?
At 15°C a 1.00 L container contains 9.91 mol N2 and 3.88 mol Ar. What is the partial pressure of each gas, and what is the total pressure inside the container? HOW DO WE GET THERE? What is the partial pressure of N2? atm
4. (10 pts) A balloon is filled with 2.16 mol of He and 1.62 mol N2 and is at -4.00°C. If the balloon is spherical what is the diameter? Assume that when inflated the atmospheric pressure is 0.98987 atm.
A mixture of gases contains 0.290 mol CH4, 0.270 mol C2H6, and 0.280 mol C3H8. The total pressure is 1.45 atm. Calculate the partial pressures of the gases. (a) CH4 (b) C2H6 (c) C3H8 in atm
for this question A sample of gas contains 0.1900 mol of N2(g) and 0.3800 mol of H2(g) and occupies a volume of 20.6 L. The following reaction takes place: N2(g) + 2H2(g) —>NH49) Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant L A sample of krypton gas collected at a pressure of 1.40 atm and a temperature of 26.0 °C is found to occupy a volume of 28.8...