Consider the reaction: Cl2(g)+3F2(g)→2ClF3(g) Δ[Cl2]/Δt = -0.052 mol L−1 s−1 . Find Δ[F2]/Δt Find Δ[CIF3]/Δt Find the rate of the reaction.
Consider the reaction: Cl2(g)+3F2(g)→2ClF3(g) Δ[Cl2]/Δt = -0.052 mol L−1 s−1 . Find Δ[F2]/Δt Find Δ[CIF3]/Δt Find...
Consider the reaction: Cl2(g)+3F2(g)→2ClF3(g) Δ[Cl2]/Δt = -0.012 M/s . 1)Find Δ[F2]/Δt 2)Find Δ[ClF3]/Δt 3)Find the rate of the reaction.
Consider the reaction: Cl2(g)+3F2(g) +2C1F3(g) A[Cl2]/At = -0.098 M/s. Part A Find A[F2]/At Express your answer to two significant figures and include the appropriate units. μΑ ? A[F]/At = Value Units Submit Request Answer Part B "Find ACIF3]/At Express your answer to two significant figures and include the appropriate units. HA ? A[CIF 31/At = Value Units Part Find the rate of the reaction. Express your answer to two significant figures and include the appropriate units. μΑ ? Rate =...
Question 1 2 pts What is the equilibrium expression for the reaction 3F2(g) + Cl2(g) <--> 2 CIF3(g)? K=... O 2[CIF3/3[F][Cl] O [CIF/[F][CI] O [CIF31/[F8[CI O none of these
Chlorine gas reacts with fluorine gas to form chlorine trifluoride. Cl2 (g) + 3F2 (g) > 2CLF3 (g) A 2.00 L reaction vessel, intially at 298K, contains Cl2 gas at a partial pressure of 337 mmHg and F2 gas at a partial pressure of 729 mmHg. Identify the limiting reactiant and determine the theoretical yield of ClF3 in grams. What is the final pressure in the reacion vesseul assuming its volume and temperatue remain constant.
Consider the reaction 8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/Δt = -0.067 M/s You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Part A Find Δ[O2]/Δt. Express your answer to two significant figures and include the appropriate units. Δ[O2]/Δt = StartFraction Upper M Over s EndFraction Previous AnswersRequest Answer Incorrect; Try Again; One attempt remaining Part BPart complete Find Δ[H2O]/Δt. Express your answer to two significant figures and include the appropriate units. Δ[H2O]/Δt = 6.7×10−2 Ms Previous Answers Correct...
4) Given the thermochemical equations: (3 points) Br2(l) + F2(g) → 2BrF(g) Br2(1) + 3F2(g) → 2BrF3(g) AH°= -188 kJ/mol AH°= -768 KJ/mol Calculate the AH°rxn for the reaction BrF(g) + F2(g) → BrF3(9)
Consider the reaction: Cl2(9)+3F (9) +2C1F3 (9) A[Cl]/At = -0.098 M/s. Find A[F2]/At Express your answer to two significant figures and include the appropriate units. Part B Find A(CIF3]/At Express your answer to two significant figures and include the appropriate units. Part C Find the rate of the reaction. Express your answer to two significant figures and include the appropriate units.
Consider the reaction 8H2S(g)+4O2(g)→8H2O(g)+S8(g)8H2S(g)+4O2(g)→8H2O(g)+S8(g) Δ[H2S]/ΔtΔ[H2S]/Δt = -0.022 M/sM/s You may want to reference (Pages 587 - 592) Section 14.3 while completing this problem. Part A Find Δ[O2]/ΔtΔ[O2]/Δt. Express your answer to two significant figures and include the appropriate units. Part B Find Δ[H2O]/ΔtΔ[H2O]/Δt. Express your answer to two significant figures and include the appropriate units. Part C Find Δ[S8]/ΔtΔ[S8]/Δt. Express your answer to two significant figures and include the appropriate units. Part D Find the rate of the reaction. Express...
2501 b) 254 g c) 266 g 270 g e) 286 g Pls PT 3 PI 3 0.6567 m Y O.985 PI 3 e 0-656X 4111621/mol 970.33 Yield is 98.S 970-33x . Jrang The reaction of 5.0 g of F2 with excess Cl2 produced 5.6g of CIF3. What is the percent yield of the reaction?F2 38.00 g/mol, CIF3 = 92.45 g/mol Cl2+3F2 2CIF a) 92% b) 58% c) 69% d) 76% e) 86% For questions 9-12, use the following equation...
Consider the equilibrium reaction Ti(s) + 2 Cl2(g) left right arrow TiCl4(l). Initially, 0.85 mol of Ti(s) 1.5 mol Cl2(g), and 17.0 mol TiCl4(l) are added to a 1 L vessel at 2472 °C and the reaction is allowed to achieve equilibrium. Given Kc = 100, which of the following corresponds to the equilibrium Cl2 concentration? Quadratic equation: x = fraction numerator negative b space plus-or-minus square root of b squared minus 4 a c end root over denominator 2...