Given the following regression lines, calculate T_i and T_f if a reactant was added at t=3.5 min
T= 0.10013*t + 16.46245
T= -0.14998*t + 30.00143
Which equation is used to calculate T_i? Which is used to calculate T_f?
Calculate T_i and T_f
Calculate Hfor the reaction: NH3(g)+5O2(g)->4NO(g)+6H2O(g)
N2(g)+O2(g)->2NO(g)
N2(g)+3H2(g)->2NH3(g)
2H2(g)+O2(g)->2H2O(g)
Compound |
Hf(kJ/mol) |
H2(g) |
0.00 |
H2O(g) |
-241.83 |
N2(g) |
0.00 |
NH3(g) |
-45.94 |
NO |
+90.2 |
O2(g) |
0.00 |
What’s the purpose of a calibration curve?
What causes absorption?
QUESTION NO. 4 is incomplete
Given the following regression lines, calculate T_i and T_f if a reactant was added at t=3.5...
Exercise C For each of the reactions listed below. use the reactions after it to determine the enthalpy of the first reaction. Reaction 1 Find the AH for the reaction below. given the following reactions and subsequent AH values: 4 NH3(g) + 5O2(g) - 4NO(g) + 6H2O(g) N2(g) + O2(g) - 2NO(g) AH = +180.6 kJ N2(g) + 3H2(g) + 2NH3(g) AH = -91.8 kJ 2 H2(g) + O2(g) 2H2O(9) AH = -483.7 kJ Reaction 2 Find the AH for...
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. 2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M (d) 2SO3(g)⇌2SO2(g)+O2(g)KP=16.5; SO3 = 1.00...
Answer the following questions ans please show your calculation. = 24,7 +402.8 = 1 AH,º= -447KJ AH2O= -484KJ AH;O= -429KJ AHRO= HW12 Using the following reactions: A+B+ 2C LA +3D+ 2E 2D+B+ 2F Calculate AH for the process 4E+ 5B → 4C +6F HW13 Using the following reactions: N2(g) + O2(g) → 2NO(g) N2(g) + 3H2(g) + 2NH3(g) 2H2(8) + O2(g) → 2H20(8) Calculate AH for the process 4NH3(g) + 502(8) → 4NO(g) + 6H2O(8) AH =+180.6 kg AH,O= -91.8...
Given the following data for heats of reaction N2(g) + 3H2(g) ----> 2NH3(g) H = -91.8 kJ C(graphite) + 2H2(g) -------> CH4(g)H = -74.9kJ H2(g) + 2C(graphite) + N2(g) --------> 2HCN(g) H = 270.3 kJ Calculate H for the reaction used to make HCN CH4(g) + NH3(g) --------> HCN(g) + 3H2(g)
URGENT Given the following data, calculate the enthalpy change of combustion for 2.5mol of nitromethane. [5A] overall reaction: 4CH3NO2(g)+3O2(g)-->4CO2(g)+2N2(g)+6H 20 (1) C(g)+O2(g)-->CO2(g) AH=-393.5k) 2H2(g)+O2(g)--> 2H2O(g) AH=-483.6k) 2C(8)+3H2(g)+2O2(g)+N2(g)-->2CH3NO2(g) AH=-226.2k)
17.51 Calculate the entropy change for the following processes. (a) 1.00 mol H,O(s) melts at 0 °C. AH = 6.01 kJ/mol. (b) 2.00 mol CH.() vaporizes at 80.0 °C. AH vap = 30.7 kJ/mol. 17.52 - Calculate the entropy change for the following processes. (a) 2.00 mol NH3(e) vaporizes at -33.0 °C. AHvap = 23.35 kJ/mol. (b) 1.00 mol C,H,OH(s) melts at -114 °C. AHjus = 5.0 kJ/mol. 17.53 Use data from Appendix G to calculate the standard entropy change...
3) The following are at constant T and P. The conditions described in (a) and (b) are initial conditions. Calculate Qc and CLEARLY indicate, with an arrow (">", or "+") to which side the reaction must shift in order to attain equilibrium. (a) A 500.0-ml flask containing 0.0500 mol of NO(g), 0.0155 mol of Cl2(g), and 0.500 mol of NOCI: 2NO(g) + Cl2(g) 2NOCI(g) K = 4.6 x 104 (b) A 2.00-L flask containing 35.0 g of NH3, 20.0 g...
3) The following are at constant T and P. The conditions described in (a) and (b) below are initial conditions. Calculate Qc and CLEARLY indicate, with an arrow ("", or " to which side the reaction must shift in order to attain equilibrium. (a) A 250.0-ml flask containing 0.0250 mol of NO(g), 0.0100 mol of Cl2(g), and 0.250 mol of NOCI: 2NO(g) + Cl2(g) O 2NOCI(g) K= 4.6 x 10 (b) A 5.00-L flask containing 35.0 g of NH3, 20.0...
The general form of a chemical reaction is aA + bB = cC +dD Where A and B are reactants in the forward direction and C and D are products in the forward direction. The lower case letters are the stoichiometric coefficients for the balanced equation. The general form of the equilibrium constant equation is then: Keq = [C]c[D]d/[A]a[B]b Part I: Q vs. K Q: reaction quotient can be calculated for a reaction at any concentration values of reactants and...
True or False t. For an exothermic reaction, the equilibrium constant, Kc, becomes smaller as the temperature increases and larger as the temperature decreases. u. The gas-phase equilibrium shown below is used to produce ammonia, NH3, for commercial applications. The NH3 yield can be increased by decreasing the temperature, increasing the pressure, and removing some NH; from the mixture. N2(g) + 3H2(g) - 2NH3() AH = -94 kJ. v. For the gas-phase equilibrium described above (see problemlu), an increase in...