=> -½ ∆[N2O]/∆t ---> the -ve sign
indicate that the concentration is decreasing.
N2O must be a reactant and 1/2 indicate that there r 2 moles of N2O
undergoing reaction.
=> ∆[O2]/∆t ---> the +ve sign
indicate that the concentration is increasing.
O2 must be a product and 1 indicate that there is 1 moles of O2
being produced
=> ½ ∆[N2]/∆t ---> the +ve
sign indicate that the concentration is increasing.
N2 must be a product and 1/2 indicate that there is 2 moles of N2
being produced.
Therefore, the balanced reaction is 2N2O ---> 2N2 + O2
10) Write a balanced reaction for which the following rate relationships are true. 1 Δ[N2] =...
Write a balanced reaction for which the following rate relationships are true: Rate = -1/2 delta[N2O5] over delta t = 1/4 delta[NO2] over delta t = delta]O2] over delta t a. 2N2O5 yields 4NO2 + O2 b. 4NO2 + O2 yields 2N2O5 c. 2N2O5 yields NO2 + 4O2 d. 1/4 NO2 + O2 yields 1/2 N2)5 e. 1/2 N2O5 yields 1/4 NO2 + O2 Can someone please describe WHY the answer is A? Please show work.
1 points Save Answe QUESTION 8 Choose the balanced reaction for which the following rate relationships are true. -A[N2O5] A[NO2] 4[NO2] 4[02] rate 2 At 4Δt Δt 2 N 205 - NO 2 + 402 01/21 2015 - / NO 2 + 02 2 N 205 4 NO 2 + O2 4 NO 2 + O2 2 N 205 NO 2 +02 - įN 205
Write a balance reaction for which the following rate relationships are true.Rate=1/2Δ(N2)/Δt=Δ(O2)/Δt=-1/2Δ(N2O)/ΔtA. 1/2N2+O2-->1/2N2OB.2N2O-->2N2+O2C.N2O-->N2+2O2D.1/2N2O-->1/2N2+O2E.2N2+O2-->2N2O
both please What is the chemical equation corresponding to the heat of formation (AH, (C2H6 (9)) of ethane(C2H6(g))? 2C(s) + 3H2(g) - C2Holg) CzHole) +2C(s) + 3H2(8) 2C2H6(g) +702(g) + 4CO2(g) + 6H20(1) 2C(s) + 6H(g) —C2Hole) Question 9 1 pts Write a balanced reaction for which the following rate relationships are true. Rate - D - 00:0) = + 41231 = + 2010.) N2+O2 ® N20 N20 ® N2 + 202 N20 ® Nz+202 2 N2 + O2 ®...
- When the following reaction is at equilibrium, which of these relationships is always true? Se 2 03(g) = 3 O2(g) -) K[O3)2 = [O213 str(0.5 pt) 3) [03] = [O2] SEP ) Kc[02]2 = [03] ) K[02]3 = [O3)2 S -) [O3)2 = [02]3.
The Haber reaction for the manufacture of ammonia is: N2 + 3H2 → 2NH3 Without doing any experiments, which of the following can you say MUST be true? True False The reaction is not an elementary reaction. True False The reaction is first order in N2. True False Δ[H2]/Δt will have a positive value. True False Reaction rate = -Δ[N2]/Δt. True False Disappearance rate of N2 = 3 (Disappearance rate of H2). True False Disappearance rate of H2 = 3 (Disappearance rate of N2). True False The...
The Haber reaction for the manufacture of ammonia is: N2 + 3H2 → 2NH3 Without doing any experiments, which of the following can you say MUST be true? The reaction is not an elementary reaction. The activation energy is positive. Disappearance rate of N2 = 3 (Disappearance rate of H2). Δ[H2]/Δt will have a positive value. Disappearance rate of H2 = 3 (Disappearance rate of N2). Reaction rate = -Δ[N2]/Δt. The reaction is first order in N2.
a) Which of the following is NOT a rate? kg/hour mol/g mol/second g/minute b) Which is a valid way to express reaction rate for N2(g) + 3 H2(g) → 2 NH3(g)? rate = - Δ[N2]/Δt, rate = -1/3 Δ[H2]/Δt, rate = 1/2 Δ [NH3]/Δt rate = Δ[N2]/Δt, rate = 1/3 Δ[H2]/Δt, rate = -1/2 Δ [NH3]/Δt rate = - Δ[N2]/Δt, rate = -3 Δ[H2]/Δt, rate = 2 Δ [NH3]/Δt rate = Δ[N2]/Δt, rate = 3 Δ[H2]/Δt, rate = -2 Δ...
For the reaction: N2(g) + H2(g) → NH3(g) (balanced?) ; If the rate of decrease of N2 is -0.11M/s what is the rate of increase of NH3?
2) A proposed reaction mechanism for nitric oxide, NO, produced in hydrogen fueled jet engines 1s 2 NO(g) N202(g) N202(g) + H2(g) H20(g) +N20(g) N20(g) +H2(g) N2(g) + H20(g) fast slow fast a) Write a balanced equation for the overall chemical reaction (1/2 mark) b) Determine the theoretical rate law. (1 mark) c) Using the blank reaction progress diagram below sketch the energy profile of this exothermic reaction mechanism, labeling the positions of NO. H2,N 02, N2O, H2O, N2. (3...