1) Given the following balanced equation, determine the rate of reaction with respect to [H2]. N2(g)...

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1) Given the following balanced equation, determine the rate of reaction with respect to [H2]. N2(g) + 3 H2(g) → 2 NH3(g) 2) Write a balanced reaction for which the following rate relationships are true. 1 A[N205] 1 A[NO2] Δ[02] 2 At 4 At = At Rate = - = 3) Given the rate law for reaction below: NO(g) + 03 (g) → NO2(g) + O2(g) Rate = K[NO][03] What is the order with respect to NO concentration? What is the order of reaction overall? [BrO3] is doubled? [Br] is reduced in half? [H*] is increased quadrupled? 4) Given the rate law: Rate = k[BrO3 ][Br][H*]², by what factor does the rate of reaction increase when: 5) Given the rate law, Rate = k[NO₂]²[Cl₂], what would be the units of k if the rate is expressed as M/s ? Hint, remember all units in rate laws need to be consistent and units of concentrations are in M.) 6) Consider the reaction, Cl₂(g) + 3 F₂(g) → 2 CIF3(g). At the start of this reaction, 0.036 mol Cl₂ was consumed in a 3.0 L container per second of reaction. a. What is the rate of consumption of the Cl₂ in M/s? b. What is the rate of production of CIF3 in M/s? c. What is the rate of consumption of F₂ in M/s? d. What is the initial rate of reaction in M/s? 1) Given the following balanced equation, determine the rate of reaction with respect to [H2]. N2(g) + 3 H2(g) → 2 NH3(g) 2) Write a balanced reaction for which the following rate relationships are true. 1 A[N205] 1 A[NO2] Δ[02] 2 At 4 At = At Rate = - = 3) Given the rate law for reaction below: NO(g) + 03 (g) → NO2(g) + O2(g) Rate = K[NO][03] What is the order with respect to NO concentration? What is the order of reaction overall? [BrO3] is doubled? [Br] is reduced in half? [H*] is increased quadrupled? 4) Given the rate law: Rate = k[BrO3 ][Br][H*]², by what factor does the rate of reaction increase when: 5) Given the rate law, Rate = k[NO₂]²[Cl₂], what would be the units of k if the rate is expressed as M/s ? Hint, remember all units in rate laws need to be consistent and units of concentrations are in M.) 6) Consider the reaction, Cl₂(g) + 3 F₂(g) → 2 CIF3(g). At the start of this reaction, 0.036 mol Cl₂ was consumed in a 3.0 L container per second of reaction. a. What is the rate of consumption of the Cl₂ in M/s? b. What is the rate of production of CIF3 in M/s? c. What is the rate of consumption of F₂ in M/s? d. What is the initial rate of reaction in M/s?