The pressure of O2 in a 1.00 L container at 20.0 °C is 0.370 atm. What...
11 point) The pressure of O2 in a 1.00 L container at 20.0 °C is 0.370 atm. What will the pressure inside the container be if 0.0100 mol CO2 is added to it? 0.380 atm 0.241 atm 1.01 atm O 0.611 atm Question 13 (1 point) ✓ Saved Consider the following phase diagram: P (atm) 3 0 10 20 30 40 50 60 70 TIC) What state of matter exists in the current room conditions? liquid 0 0 solid sas
A quantity of N2 gas originally held at 3.80 atm pressure in a 1.00 L container at 26.0ºC is transferred to a 10.0 L container at 20.0ºC. A quantity of O2 gas originally at 4.75 atm and 26.0ºC in a 5.00 L container is added to the 10.0 L container already containing the N2. a) Draw a diagram outlining this experiment, labeling the various quantities. b) Calculate the total pressure in the new container. c) What is the mole fraction...
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
A sealed container with a volume of 2.00 L contains 30.0 atm of pure O2 and 1.35 g of methanol (CH3OH, 32.05 g/mol) at 25 °C. The combustion finishes, and the container is cooled back to 25 °C. What is the final partial pressure of CO2? What is the final total pressure? (20 pts) please give a detailed explanation
Part A The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 99 ∘C ? Express your answer with the appropriate units. Part B At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 35 ∘C ? Express your answer...
Part A The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 88 ∘C ? Express your answer with the appropriate units. Part B At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ? Express your answer...
Assume that you have 1.10 g of nitroglycerin in a 3000 mL steel container at 20.0°C and 1.00 atm pressure. An explosion occurs, raising the temperature of the container and its contents to 425 °C. The balanced equation is 4 CH: N30,(1) + 12 CO2(g) + 10H2O(g) + 6 N2(g) + O2(9) (Figure 1) Part A How many moles of nitroglycerin were in the container originally? 190 AU O ? TICHNO, = Submit Request Answer Part B How many moles...
A sample of O2 with volume of 20.0 L at 25°C and 1.00 atm is reacted with excess N2 to produce NO. The equation for the reaction is O2(g) + N2(g)=2NO(g) how many grams of NO are produced?
1. a. The pressure inside a hydrogen-filled container was 2.10 atm at 21 ∘C. What would the pressure be if the container was heated to 87 ∘C ? b. At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 ∘C ? c. Calculate the number of molecules in a deep breath of...
1. The Henry’s Law constant for O2 is 770 L atm mol-1 at 25 °C. What mass of oxygen would be dissolved in a 40-L aquarium at 25 °C, assuming an atmospheric pressure of 1.00 atm, and that the partial pressure of O2 is 0.21 atm? 2.The carbon dioxide concentration in a bottle of club soda is 0.12 mol L-1 at 25 °C. What is the pressure of carbon dioxide in the headspace? The Henry’s Law constant for CO2 at...