For experiments 1, 2, and 3, substituting appropriate values for the Concentrations and Rates from Table 2 into equation (3), calculate values for the orders m and n. Also determine the value of the Rate Constant k (with Units!)at room temperature of 17C. Show all calculations below

[References) Use the References to access important values if needed for this question. The reaction for the formation of phosgene from carbon monoxide and chlorine CO + C1→COCI, is first order in CO and first order in Cl,. Complete the rate law for this reaction in the box below. Use the form k[A]™[B]"... , where 'l' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 1.73x10 28 Ms1 Using this value for the rate constant, the rate of the reaction when [CO) = 2.49 M and [Cl,] 0.405 M would be Ms Submit Answer Try Another Version 2 item attempts remaining

The reaction of UO,* with hydrogen ion in aqueous solution 2 UO,* + 4 H* → U** + UO2²* +2 H2O is second order in UO,* and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A]™[B]"... , where 'l' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate =

The reduction of nitric oxide with hydrogen 2NO+2H₂ → N₂ + 2H₂O is second order in NO and first order in H₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate of the reaction was determined to be 7.99 x 10-³ M-s¹, when [NO] = S = 0.192 M and [H₂] = 0.129 M. From this experiment, the rate M².s¹. constant is