For the reaction: N2O (g) + NO2 (g) <--> 3 NO(g) , Kc = 4.2 x 10-4 at 500. K.
What is Kp for the reaction at this temperature?
Find the value of the equilibrium constant, Kp, for the following reaction N2O(g) + NO2(g) → 3NO(g) at 900 K given the following data: N2O(g): AGfº=149.2 kJ/mol; NO2(g): AGfº=89.4 kJ/mol; NO(g): AGfº=79.0 kJ/mol. 0.192 1.21 1.00 0.826 O 1.43
The Kc for the reaction at 298 K is given N2O4(g) ⇋ 2 NO2(g) Kc = 5.9 × 10–3 What is the Kc for the following reaction? ½ N2O4(g) ⇋ NO2(g) Kc = ?
3. Calculate AH for the reaction Ato AL120103 N2O(g) + NO2(g) → 3 NO(g) from the following enthalpies of reaction: NO(g) + O2(g) + NO2() N2O(g) + N2O) + O2(8) 1 N2(g) + O2(g) → NO(g) AH = -56.6 kJ AH = -81.6 kJ AH = +90.4 k]
12. The equilibrium constant for the reaction: SO2(g) + O2(g)so,(g) is Kc # 1.3 x 10, What is the equilibrium constant for the reaction: 2S0,(g)O,(g)+ 2S02(g) 13. For the following reaction, Kc (@ 500 K) 1.0 x 10 2 SO-(g) + 02(g) 2 SO,(g). What is the value of Kp for this reaction at 500 K? (3 Pts.)
1) Kc = 45 for the equilibrium : 2 NO2(g) <====> N2O4 (g) at a temperature 85 C a) What is Kc for N2O42 <====> NO2(g) ? b) What is Kp for 2 NO2(g) <====> N2O4 (g) at 85 C? R= 0.0821 L-atm/ k-mol 2) The pH of seawater is 8.10 This corresponds to ________ M H+
Under what conditions will the following reaction be the most product-favored? N2O(g) + NO2(g) <==> 3 NO(g) ; H = + 156 kJ A. low pressure, low temperature B. high pressure, low temperature C. high pressure, high temperature D. low pressure, high temperature
23 A) For the reaction 2CH4(g)⇌C2H2(g)+3H2(g) Kc = 0.130 at 1651 ∘C . What is Kp for the reaction at this temperature? 23 B) For the reaction N2(g)+3H2(g)⇌2NH3(g) Kp= 3.40×10−3 at 292 ∘C. What is Kc for the reaction at this temperature? Part A For the reaction 2CH (g) = C2H2(g) + 3H2(g) Kc = 0.130 at 1651 °C. What is K, for the reaction at this temperature? Express your answer numerically. View Available Hint(s) V AC ? K Kp...
8) The rate law for the following reaction N2O(g) + NO2(g) → 3NO(g) is Rate = k [N2O][NO2]2. Fill in the blank in the table below. Experiment [N2O], M [NO2], M Initial Rate, MS-1 1 0.100 0.100 2.0x10-3 2 0.300 0.100 6.0x10-3 3 0.100 0.200 ? a) 2.0x10−3 Ms−1 b) 4.0x10−3 Ms−1 c) 8.0x10−3 Ms−1 d) 6.0x10-3 Ms-1 e) 1.0x10−2 Ms−1
1 2 Part A Calculate Kp at 298 K for the reaction NO(g) + + O2(g) → NO2 (g) assuming that AH is constant over the interval 298-600 K. Kp = 2.31x106 Submit Previous Answers ✓ Correct Part B Calculate Kp at 477 K for this reaction assuming that AHR is constant over the interval 298-600 K. PO AQ * o o ? Kp = | Submit Previous Answers Request Answer Revie For the reaction 2CH4 (g) = C2H2(g) +...
22 A) For the reaction 2A(g)+3B(g)⇌C(g) Kc = 40.0 at a temperature of 165 ∘C∘ Calculate the value of Kp 22 B) For the reaction X(g)+2Y(g)⇌2Z(g) Kp= 1.87×10−2 at a temperature of 67 ∘C Calculate the value of Kc Part A For the reaction 2A(g) + 3B(g) = C(g) Kc = 40.0 at a temperature of 165 °C. Calculate the value of Kp. Express your answer numerically. View Available Hint(s) | ΑΣφ ? Submit Part B For the reaction X(g)...