Determine the pressure of N2 under the following conditions. 31.5 g at 15.5°C in 7.20 L
Determine the pressure of N2 under the following conditions. 31.5 g at 15.5°C in 7.20 L
Determine the pressure of N2 (in atm) under the following conditions. 0.91 mol at 34°C in 20.7 L atm
N2(g) + 3H2(g) = 2NH3(g) AH° = .92 kJ Select the conditions under which the yield of ammonia is the highest. High temperature and high pressure High temperature and low pressure Low temperature and high pressure Low temperature and low pressure
Gibbs free energy is -32.7 kJ per mole of N2 for this rxn under standard conditions: N2(g) + 3H2(g) <—> 2NH3(g) Calculate Gibbs free energy for the same rxn under these nonstandard conditions: Pressure of N2=2.00 atmospheres Pressure of H2=7.00 atmospheres Pressure of NH3= 0.021 atmospheres Temperature= 100 degrees Celsius
Under which of the following initial conditions would the reaction 2 H2O2(l) 2 H2O(l) + O2(g) NOT be able to acheive equilibrium? a. H2O2(l) is added to the flask. b. H2O2(l) and H2O(l) are added to the flask. c. H2O2(l) and O2(g) at a pressure larger than Kp are added to the flask. d. They can all achieve equilibrium.
1.The solubility of O2 in water is 0.590 g/L at an oxygen pressure of around 15.5 atm. What is the Henry's law constant for O2 (in units of mol/L
AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g) This calculation was for the reaction under standard conditions—that is, with all gases present at a partial pressure of 1 atm and a temperature of 25°C. Calculate AG for the same reaction under the following nonstandard conditions: . PN2 = 2.00 atm, PH2 = 7.00 atm, PNH3 = 0.021 atm, . and T = 100°C.
If the temperature of a 15.5 mL sample of N2 gas is increased from 25.0 °C to 75.0 °C as its pressure remains constant, what will be its new volume in milliliters? How many moles of chlorine gas at 120. °C and 33.3 atm would occupy a vessel of 12.0 L? D
N2(g) effuses at a rate that is_times that of Cl2(g) under the same conditions. Number rate ratecı
For the gas N2 calculate the volume in mL if 189 g were under a pressure of 543 torr at 40.0 oC. A sample of gas contains 62.0 moles at 327 K in 4.00 L of volume. What is the pressure (in atm) of the gas? What is the density (in mg/mL) of a H2S gas at 12.9 atm and 137 K Place the following gases in order of increasing average molecular speed at 25 oC: Slowest → Fastest energy...
Question 22 (3 points) Determine the total pressure of a mixture of 30.0 g of N2, 54.4 g of O2, and 13.3 g of H2 in a 3.00 L container at a temperature of 300.0°C Your Answer: Answer units