A mixture of an equal number of moles of N2 and H2 is contained in a 5 litre reaction chamber. The initial total pressure of the mixture at 25°C is 3 bar. When the mixture reacts to the fullest extent to form NH3, the final total pressure in bar in the chamber at 25°C is:
2.00
1.00
2.50
3.00
1.50
A mixture of an equal number of moles of N2 and H2 is contained in a...
If you mix 2.00 moles of H2, 1.00 moles of N2 and 2.00 moles of NH3 in a one liter vessel at 472 C. Will H2 and N2 react to form NH3?
A mixture of 0.0500 moles of H2 and 0.0250 moles of O2 is contained in a balloon with a volume of 30.0 mL. If the atmospheric temperature is 298 K, what is the total pressure in the balloon?
A mixture of 75% H2 and 25% N2 (molar basis) is contained in a tank at 800 atm and -70°C. Estimate the specific volume of the mixture in L/mol using Kay’s rule. H2: Tc= 33.3 & Pc=12.8 N2: Tc=126.2 & Pc=33.5
A mixture of gases contains 10.30 g of N2, 1.88 g of H2, and 7.90 g of NH3. The total pressure of the mixture is 1.80 atm. a. What is the partial pressure of N2? b. What is the partial pressure of H2? c. What is the partial pressure of NH3?
A vessel of volume 22.4 dm3 contains 2.0 mol H2 and 1.0 mol N2 at 273.15 K initially. All the H2 reacted with sufficient N2 to form NH3. Calculate the partial pressures and the total pressure of the final mixture.
A 5.0L container holds 1.5 mmol of N2 and 3.00 mmol of H2 at a total pressure of 2.00 kPa. Calculate the number of N2-H2 collisions that occur in the mixture in 1.0 ms.
A mixture of gases contains 1.26 g of N2, 3.71 g of H2, and 1.87 g of NH3. If the total pressure of the mixture is 1.67 atm, what is the partial pressure of each component? PN2 = ? atm PH2 = ? atm PNH3 = ? atm
A mixture of gases contains 8.55 g of N2, 5.51 g of H2, and 1.38 g of NH3. If the total pressure of the mixture is 3.07 atm, what is the partial pressure of each component? PN2 = _____ atm PH2 = _____ atm PNH3 = ______atm
A mixture of gases contains 1.26 g of N2, 8.57 g of H2, and 7.28 g of NH3. If the total pressure of the mixture is 1.66 atm, what is the partial pressure of each component? PN2 = atm PH2 = atm PNH3 = atm
The following ia a balanced reaction N2 (g) + 3 H2 (g)2 N We read the above reaction as follows: 1 mole of N2 (nitrogen)reacts with 3 moles of H2 (hydrogen) to form 2 moles of NH3 (ammonia). Which statement is correct (a) 14.0 g of nitrogen reacts with reacts with 6.0 g of hydrogen to form 34.0 g ammonia (b) 28.0 g of nitrogen reacts with 6.0 g hydrogen to form 17.0 g ammonia (c) 14.0 g of nitrogen...