The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 - CH4 + H2 + CO s 3.2x10-4 s-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.359 atm. What is the pressure of the system after 3.2 min? Assume ideal-gas behavior. 49 atm

The first-order rate constant for the gas-phase decomposition of dimethyl ether, (CH3)20 - CH4 + H2 + CO s 3.2x10-4 s-1 at 450°C. The reaction is carried out in a constant-volume container. Initially, only dimethyl ether is present, and the pressure is 0.359 atm. What is the pressure of the system after 3.2 min? Assume ideal-gas behavior. 49 atm

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

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.
The decomposition of dimethyl ether, (CH3)2O, at 510 °C is afirst-order process with a rate constant of 6.8x 10-4 s-1:(CH3)2O(g)------>CH4(g) + H2(g) + CO(g)If the initial pressure of (CH3)2O is 135 torr, what is its pressureafter 1420 s?
At a certain temperature the rate of this reaction is second order in H₂CO3 with a rate constant of 2.75Ms H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.130M. Calculate how long it takes for the concentration of H₂CO3 to decrease to 0.0286 M. You may assume no other reaction is important. Round your answer to 2 significant digits. X ? S
Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, g) +F, (g) NO,F (g) +F (g) k1 2 F (g) + NO, (g) → NO,F (g) k2 Suppose also k, « k,. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. rate = k U Note: your answer should not contain the concentrations of any intermediates.
The first-order reaction, 2 N2O(g) → 2 N2(g) + O2(g), has a rate constant equal to 0.76 s-1 at 1000 K. How long (in sec) will it take for the concentration of N2O to decrease to 42% of its initial concentration?
b Sulfuryl chloride undergoes first-order decomposition at 320.°C with a half-life of 8.75 h (k = 2.20 x 10-5 s1). So,Cl2(g) → SO2(g) + Cl2(g) If the initial pressure of S02CI2 is 791 torr and the decomposition occurs in a 1.25-L container, how many molecules of SO2CI, remain after 11.7 h? molecules SO2CI2
The reaction of NO and O2 produces NO2.2 NO(g) + O2(g) → 2 NO2(g)The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a giventemperature, the rate constant, k, equals 4.7  102 M–2s–1. What is the rate of reaction when the initialconcentrations of NO and O2 are 0.025 M and 0.015 M, respectively?a. 2.6  10–3 M/sb. 4.4  10–3 M/sc. 0.18 M/sd. 2.0  10–8 M/se. 3.8  102 M/s
The decomposition of N2O5 in solution in carbon tetrachloride is a first-order reaction. 2N2O5 → 4NO2 + O2 The rate constant at a given temperature is found to be 5.25 x 10-4 s-1. If the initial concentration of N2O5 is 0.24 M, what is its concentration after exactly 9 minutes have passed? Round your answer to 2 decimal places.