Example: The decomposition of NO2 at a moderately high temperature (between 300-400°C) +O2(g) 2NO(g) 2NO2( At 330...
The decomposition of NO2 at high temperature NO2(g) → NO(g) + 1/2 O2(g) is a second order process with a rate constant of 3.40 L/mol•min. If an experiment is performed where the initial concentration of NO2 is 0.400 M, what is the concentration of NO2after 2.96 min? [NO2] = M
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
Consider the reaction for the production of NO2 from NO: 2NO(g)+O2(g)→2NO2(g) 1. If 85.3 L of O2(g), measured at 38.0 ∘C and 639 mmHg , is allowed to react with 150 g of NO, find the limiting reagent. 2. If 95.7 L of NO2 forms, measured at 38.0 ∘C and 639 mmHg , what is the percent yield?
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C. How long would it take for the concentration of NO2 to decrease from 0.62M to 0.28M?
Consider the equilibrium reaction at 100°C:2NO(g) + O2(g)⇌ 2NO2(g); KC = 30,000Write the concentration equilibrium equation for the reaction. If 46 grams of NO2(g) is introduced into a 1 L flask what will be the equilibrium concentrations of NO2, O2 and NO?
The first-order rate constant for the decomposition of N2O5, N2O5(g) 2NO2(g) + O2(g)At 70C is 6.810-3s-1. Suppose we start with 0.0250 mol of N2O5(g) in a volume of 1.0 L. a.) How many moles of N2O5will remain after 2.5 min? b.)How many minutes will it take for the quantity of N2O5to drop to 0.010 mol? c.What is the half-life of N2O5at 70 degrees C?
Decomposition of NO2(g) at 300 °C yields the data in the table. Plots of In[NO2] and 1/[NO2] are shown below. The rate constant for this reaction at 300 °C is . (Hint: The units are based on the reaction order.) Report your answer with two significant figures. Do NOT include units in your answer. 2 NO2(g) → 2NO(g) + O2(g) Time (s) [NO2] (M) 0.0 0.0100 50.0 0.00787 100.0 0.00649 200.0 0.00481 300.0 0.00380 isabel Camera m o r talidad...
For the reaction 2NO(g) + O2(g) ® 2NO2(g), DH° = -113.1 kJ/mol and DS° = -145.3 J/K·mol. Under which temperature conditions would the reaction be spontaneous? _________. a. For all temperatures b. Only at high temperatures c. Only at low temperatures
2NO2(g)--2NO(g)+O2(g) (endothermic) H2(g)--2H(g) H2O(g)--H2O(l) CO2(s)--CO2(g) cem 15 Part A Predict the conditions (high temperature, low temperature, all temperatures, or no temperatures) under which each of the following reactions will be spontaneous Drag the appropriate items to their respective bins. Reset Help 2NO3(e)--2NO(g) + Os(e) (endele) - 1.00 H.) - 24(e) CO.() - CO. High temperature Low temperature All temperatures No temperatures
1a. At 573 K, gaseous NO2 decomposes, forming NO(g) and O2. If a vessel containing NO2(g) has an initial concentration of 0.056 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in the reactant, and the rate constant for this reaction, at 573 K, is 1.1 L/mol · s. = ___ s 1b. The decomposition of ammonia on a metal surface to form N2 and H2 is a zero-order reaction....