The above reaction of decomposition of 2N2O5(g) is first order reaction, the Half life of first order reaction is as follows t1/2 = 0.693/K, in this reaction the rate constant is 0.00045s-1
t1/2 = 0.693/K
t1/2 = 0.693/0.00045
t1/2 = 1540
t1/2 = 1.54 X 10-3s
12 Be sure to answer all parts. The decomposition of N_2 0_5 is described by the...
Be sure to answer all parts. The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first- order reaction: 4PH3(g) → P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. (a) Calculate the first-order rate constant for the reaction. S (b) Calculate the time required for 29% of the phosphine to decompose. S
Be sure to answer all parts.The thermal decomposition of phosphine \(\left(\mathrm{PH}_{3}\right)\) into phosphorus and molecular hydrogen is a first-order reaction:\(4 \mathrm{PH}_{3}(g) \rightarrow \mathrm{P}_{4}(g)+6 \mathrm{H}_{2}(g)\)The half-life of the reaction is \(35.0 \mathrm{~s}\) at \(680^{\circ} \mathrm{C}\)Calcnlate the first-order rate constant for the reaction:_______s-1Calculate the time required for 95.0 percent of the phosphine to decompose:_______Col
The decomposition of N2O5 is described by the following equation. 2N2O5(g) → 4NO2(g) + O2(g) If the rate constant is 2.50 × 10−4 s−1, what is the half-life of this reaction?
Be sure to answer all parts. Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AH - 117.3 kJ (a) Is heat absorbed or released in the reaction? absorbed released (b) What is A n for the reverse reaction? -1173 EJ (c) What is AH when 5.20 mol of CO, reacts with excess Mgo? (a) What is AH when 32.5 g of CO, reacts with exces: Mgo?
Be sure to answer all parts. The reaction 2A rightarrow B is second order in A with a rate constant of 32.1 M^-1 s^-1 at 25 degree C. Starting with [A]0 = 0.00779 M, how long will it take for the concentration of A to drop to 0.001803M? s Calculate the half-life of the reaction for [A]_0 = 0.00779 M. s Calculate the half-life of the reaction for [A)0 = 0.00269 M.
The decomposition of N,is described by the following equation. 2N,O3(2)→ 4NO2(8) + O2(g) If the rate constant is 4.50 x 10-45-1, what is the half-life of this reaction? * 10s (Enter your answer in scientific notation.)
Be sure to answer all parts. The gas-phase decomposition of peroxyacetyl nitrate (PAN) obeys first-order kinetics: CH3COOONO2 + CH3C000 + NO2 with a rate constant of 4.9 x 10-45-1. Calculate the rate of decomposition (in M/s) if the concentration of PAN is 0.35 ppm by volume. Assume STP conditions. rate= x 100 M/s (Enter your answer in scientific notation.)
Question 12 (of 23) - > 12. Be sure to answer all parts. Given the reaction represented by the balanced equation CH,6) +316) + 3HI(g) + CHT() Part 1: Calculate the number of g of CHI, produced by mixing 140 g 1, with excess CH- T2,4 CH Part 2 out of 2 If 49.0 g CHI, were actually produced, calculate the % yield. % yield MacBook Air
Be sure to answer all parts. The reaction 2A B is second order with a rate constant of 51.0/M-min at 24°C. (a) Starting with [Alo 8.90 x 10 M, how long will it take for [A],3.30 x 103 M? min (b) Calculate the half-life of the reaction. min
Be sure to answer all parts. For a certain reaction, the frequency factor A is 8.3 × 109 s−1 and the activation energy is 22.4 kJ/mol. What is the rate constant for the reaction at 92°C _ × 10_ s−1 (Enter your answer in scientific notation.)