first order reaction rate constant, k

Please answer ALL parts of the question and show your work. Consider this reaction: N2(g) + 3H2(g)  <------>  2NH2(g)          H= -123kJ Describe how the concentration of H2 will be affected by each of the following changes to the system at equilibrium. Will it increase, decrease, or not change? (a) The volume of the reaction chamber is decreased (b) Helium gas is added to the reaction chamber (c) The temperature is increased (d) N2 has is added to the reaction chamber

Write the balanced chemical equation for the complete combustion of heptene, C7H14. In combustion, hcpLcnc reacts with oxygen to produce carbon dioxide and water.What is the mole ratio that would enable you to calculate the number of moles of oxygen needed to react exactly with a given number of moles of heptene? What mole ratios would you use to calculate how many moles of each product form from a given number of moles of heptene?

Consider the following reactions: CaSO4(s) Ca²+ + SO4²- CaF₂(s) Ca²+ + 2F- Kso=10-4.59 Kso-10-10.3 a) What is the solubility of CaSO4(s) in water at 25 °C? b) What is the solubility of CaF2(s) in water at 25 °C? c) Will either of these two solids will precipitate if [F]=104 M, [SO4²¯]=10-³ M and [Ca²+]=10-² M?

Ozone in the upper atmosphere is decomposed by nitro- gen oxide through the reaction 03 + NO →02 + NO2 The experimental rate expression for this reaction is rate = k[O3 ][NO] Which, if any, of the following mechanisms are consistent with the observed rate expression? (a) O3 + NO –→0+NO; 0 + 03 →2 02 NO3 + NO → 2 NO2 (b) O3 + NO – 02 NO2 (c) NO+ NO=N2O2 N2O2 + O; → NO2 + 2 O2 (slow) (fast) (fast) (slow) (fast equilibrium) (slow)

The reaction in which CO2 decomposes to CO and a free radical oxygen atom, O, has an activation energy of 460 kJ mol. The frequency factor is 3.6 x 10+2 s. What is the rate constant for this reaction at 312 K? (Enter your answer to two significant figures.) Rate constant = S

The decomposition of formic acid vapor according to the following reaction at 550oC follows a first-order kinetics, and at the above temperature, the reaction has a half-life of 240 s.             HCO2H (g)   ®  CO2(g)  +  H2(g);                Rate = k[HCO2H]  If the initial concentration of HCO2H was 0.160 M, what is its concentration after four half-lives?  (A) 0.010 M                (B) 0.020 M                  (C) 0.040 M                  (D) 0.0050 M

2. Find the AH for the reaction below, given the following reactions and subsequent AH values: 2C2(g) + H2O(g) – C2H2(g) + /2 02(g) C2H2(g) + 2H2(g) C2He(g) AH = -94.5 kJ H20(g) - H2(g) + % O2 (g) AH =71.2 kJ C2H6(g) + /2 Oz(g) - 2 CO2(9) + 3 H2O(g) AH = -283 Kj

The equilibrium constant, K., for the following reaction is 1.80×10-2 at 698 K. 2HI(g) H2(g) + I2(g) Calculate the equilibrium concentrations of reactant and products when 0.341 moles of HI are introduced into a 1.00 L vessel at 698 K. [HI] M [H2] M [L] M

Nitric acid is used in the starting material for the production of ammonium nitrate. The final reaction in producing ammonium nitrate is: 3HNO,(aq) – HNO,(aq) + H,O() + 2NO(9) Using your knowledge collision theory and the factors that affect the rate of a reaction, describe 3 ways that the rate of this reaction can be increased to produce more ammonium nitrate. Include specific reasons why it would increase. (A:3)