Dinitrogen pentoxide (N2O5) decomposes as follows to nitrogen dioxide and nitrogen trioxide: $$N2​O5​(g)NO2​(g)+NO3​(g) Calculate the average rate of the reaction between consecutive measurement times in the following table.  Time (s) [N2O5] (molecules/cm3)  0.00 1.405×1012   1.85  1.331×1012  3.70  1.275×1012  5.55  1.231×1012  7.40  1.197×1012  Express every answer to two significant figures. Rate 1 =     Rate 2 = Rate 3 = Rate 4 =

Consider the reaction: N₂(g) + 3H₂(g) → 2NH₂ (g) M S Suppose that a particular moment during the reaction, molecular hydrogen is reacting at a rate of -0.0400 At what rate is ammonia being formed? Round your answer to 3 significant digits. M S 0 x10 X

C:H-Br(ag) + H2O(1) → C3H¬OH(ag) + HBr (ag) concentration of the reactant changes from 0.0671 M at 125 seconds to 0.0549 M at 315 sec. Calculate the average rate of decomposition. Write the rate for the following reaction in terms of: 2HCI(g) → H2(g) + Cl2(g) (а) HCI (b) Н

For the decomposition of nitrous oxide at 565 °C 2 N20(g) → 2 N2(g) + 02(g) the average rate of disappearance of N,0 over the time period from t = 0 s to t = 2.02×103 s is found to be 2.82×10 4 M/s. What is the average rate of appearance of 0, over the same time period? M/s.

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. = (0.291 M¹s¹) [N₂0₂] rate Suppose a vessel contains N₂O, at a concentration of 0.230 M. Calculate how long it takes for the concentration of N₂O to decrease to 23.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. ? Subm Continue Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use Privacy Cente 80°F Partly sunny ^ pe here to search B X G

2. Consider the reaction that occurs when a CIO2 solution and a solution containing hydroxide ions (OH) are mixed at 0°C, shown in the following equation. 2CIO2(aq) + 2OH (aq) → Cl03° (aq) + CIO2° (aq) + H2O (1) When solutions containing CIO2 and OH- in various concentrations were mixed at 0 oC, the following rate data were obtained: Determination Initial concentration Initial concentration of Initial rate for formation number of ClO2, mol/L OH", mol/L of CIO3¯ mol/Ls 1.25x10-2 1.30x10-3 2.33x10-4 2.50x10-2 1.30x10-3 9.34x104 3 2.50x10-2 2.60x103 1.87x10-3 a) Use the method of initial rates to find the order of the reaction with respect to CIO2 and with respect to OH. Write the rate equation for the reaction of CIO2 and OH´ at 0°C. b) Calculate the rate constant, k, for the reaction of clO2 and OH at 0°C. c) Calculate the reaction rate for the reaction CIO2 and OH at 0°C when the initial ClO2 and OH concentrations are 8.25x10-3 mol/L and 5.35x 10-² mol/L, respectively. 1.

In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!

Determine the average rate of change of B from t :0 s to Time (s) Concentration of A (M) t = 252 s. 0.740 126 0.425 A → 2B 252 0.110 rateB = M/s

Consider Following reaction: CH4(g) + 4 NO(g)  → 2 N2(g) + CO2(g) + 2 H2O(g) The concentration of NO was 3.176M at t = 0.39 s and 0.947 M at t = 7.60 s. What is the rate of consumption of CH4  in M/s? Report your answer with four decimals. Enter numbers only; do not enter units.

Dinitrogen pentoxide (N2O5) decomposes as follows to nitrogen dioxide and nitrogen trioxide:$$N2​O5​(g)NO2​(g)+NO3​(g)Calculate the average rate of the reaction between consecutive measurement times in the following table.   0.00 1.705×1012   1.45  1.616×1012  2.90  1.545×1012  4.35  1.486×1012  5.80  1.437×1012