Consider the reaction:
N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔHrxn = -92.6 kJ
Calculate the heat (in kJ) given off with the complete reaction of 17.5 grams of hydrogen gas.
Consider the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) ΔHrxn = -92.6 kJ...
Consider the following reaction. N2(g) + 3 H2(g) → 2 NH3(g) Determine the mass of N2 gas required to react with 10.85 g gaseous H2. O 13.90 g N2 150.8 g N2 32.55 g Na 3.617 g N2 50.26 g N2 O O O
For the reaction N2(g) + 3 H2(g) = 2 NH3(g), what is AG (in kJ) at 298 K when the pressures of the gases are: P(N2) .13 atm P(H2) = 6.2 x 10-5 atm P(NH3) = 1.8 atm? O +47.0 O-113 O-2.49 0 -33.0 O +1.73
Consider the reaction: N2(g) + 3 H2(g) « 2 NH3(g) a. Write the expression for the equilibrium constant, K, for this reaction. b. An equilibrium misture of N2, H2, and NH3 at 300°C is analyzed, and it is found that: [N2] = 0.25 mol/L, [H2] = 0.15 mo/L, and [NH3] = 0.090 mol/L. Find K at 300°C for this reaction.
Consider the reaction: 2 NH3 (g) → 3 H2 (g) + N2 (g) Which of the following is true about entropy associated with this reaction? A. The entropy of the system will be positive because the mol of gas is increasing. B. The entropy of the system will be negative because the mol of gas is decreasing. C. The entropy of the system will be negative because the mol of gas is increasing. D. The entropy of the system will...
Consider the reaction: N2(g) + 3 H2(g) = 2 NH3(g) Kc = 0.0043 T = 300 °C The value of Kp for this reaction is a. less than ko O b.greater than kc O c equal than ke Consider the reaction: N2 (g)+3 H2 (g)=2 NH3 (g)Kc = 0.0043T = 300 °C Part 1. Given the initial conditions below, which statement is true? [N2] = 0.015 M [H2] = 0.010 M [NH3] = 0.025 M O a. Q is greater...
1. Consider the reaction below. N2(g) + 3 H2(g) ⇋ 2 NH3(g) Which of the following changes would cause less NH3 to be produced? decreasing the volume adding N2 increasing the volume adding H2 2. Consider the following reaction. N2(g) + 3 H2(g) ⇋ 2 NH3(g) The forward reaction is exothermic. Which of the following changes would cause less NH3 to be produced? decreasing the temperature adding H2 increasing the temperature adding N2 3. What is the effect of a...
Use the following equations N2 (g) + 3 H2 (g) 2 NH3 (g) N2 (g) + O2 (g) → 2 NO (g) 2 H2 (g) + O2 (g) + 2 H20 (1) DH = -99.22 kJ DH = + 180.5 kJ DH = - 571.6 kJ to calculate the enthalpy change for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H20 (1) DH = ?
For the reaction 2 NH3 --> 3 H2 + 2 N2 The rate of disappearance of ammonia is -0.00698 M/hr Calculate the rate of appearance of hydrogen gas Calculate the rate of appearance of nitrogen gas
At 400 K, the reaction N2 (g) + 3 H2 (g) → 2 NH3 (g) reaches equilibrium when the partial pressures of nitrogen, hydrogen, and ammonia gases are 4.00 atm, 1.00 atm, and 1.05 x 10−2 atm, respectively. Given that the standard enthalpy of the reaction at 400K is DH = -94 kJ/mol, estimate the value of the equilibrium constant KP at 450 K assuming that the standard enthalpy of reaction does not vary significantly with temperature in this temperature...
5. Heat of Reaction under standard conditions : Determine the amount of heat (in kJ) given off, when 1.26 x 104 g of ammonia ( NH3 ) are produced according to the equation : N2 (g) + 3 H2 (g) → 2 NH3 (g) ....... AH ºrx = - 92.6 kJ Assume that the reaction occurs at Standard State conditions at 25 C. ANSWER : Total Heat Given Off: _ (units ?) 6. Standard Enthalpy of Formation and Reaction :...