Given: C(s) +2H2(g) → CH4(g)
If Δ[CH4]/Δt = 7.2x10-4 M/s, then -Δ[H2]/Δt is equal to ________ M/s.
Given: C(s) +2H2(g) → CH4(g) If Δ[CH4]/Δt = 7.2x10-4 M/s, then -Δ[H2]/Δt is equal to ________
The gas NO reacts with H2, forming N2 and H2O: 2NO(g)+2H2(g) 2H2O(g)+N2(g) If Δ[NO]/ Δt = –24.0 M/s under a given set of conditions, what are the rates of change of [N2] and [H2O]?
Calculate Δ Hrxn for the following reaction: CH4(g)+4Cl2(g)→CCl4(g)+4HCl(g) given these reactions and their ΔH values: C(s)C(s)H2(g)+++2H2(g)2Cl2(g)Cl2(g)→→→CH4(g),CCl4(g),2HCl(g),ΔH=−74.6 kJΔH=−95.7 kJΔH=−184.6 kJ
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)→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 at 298 K. C(graphite)+2 H 2 (g)⟶ CH 4 (g)Δ?°=−74.6 kJ C(graphite)+2H2(g)⟶CH4(g)ΔH°=−74.6 kJ Calculate the quantities. Delta Ssys=_______ J/K Delata Ssurr =_______ J/K
10. Calculate ∆Hrxn for the reaction: CH4(g) + 4Cl2 → CCl4(g) + 4HCl(g) Given that: C(s) + 2H2(g) → CH4(g) C(s) + 2Cl2(g) → CCl4(g) H2(g) + Cl2(g) → 2HCl(g) ∆H = -74.6kJ ∆H = -95.7kJ ∆H = -92.3kJ
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...
B) 1/2 N2(g) + 2H2(g) + 1/2 Cl2(g) → NH4Cl(s) C) N2(g) + H2(g) + Cl2(g) → 2 NH4Cl(s) D) N2(g) + Cl2(g) + 4 H2(g) → 2 NH4Cl(s) E) 1/2 N2(g) + 1/2 Cl2(g) + 1/2 H2(g) → NH4Cl(s) 12) Which molecule contains the most polar bonds? A) NBr3 B) CH4 C) CF4 D) CO2 The spheres below represent atoms of Li, Be, B, and F (not nece
Calculate the enthalpy of the following reaction: C (s) + 2 H2 (g) --> CH4 (g) Given: C (s) + O2 (g) --> CO2 ΔH = -393 kJ H2 + 1⁄2O2 --> H2O. ΔH = -286 kJ CH4 + 2O2 --> CO2 + 2H2O ΔH = -892 kJ
Part A Calculate Δ Han for the following reaction: C(s) +H2O(g)CO(g)+H2() Use the following reactions and given ΔΗ values: C(s) + O2 (g)- CO2 (g), ΔΗ-393.5 kJ 2CO (g) + O2 (g)--2CO2 (g), ΔΗ-566.0 kJ 2H2 (g) +02 (g)-2H3O(g). Ан :-483.6 kJ Express your answer using four significant figures. kJ Submit Request Answer