At high temperatures, A(s) decomposes to B(s) and C(g) 2A(5) 3B(s) + C(9) When the rate...
At high temperatures, A(s) decomposes to B(s) and C(g): 2A(s) 3B(s) + C(g) When the rate of formation of B(s) is 8,952 M/s, the rate of decomposition of A(s) is M/s. (Answer should be in 3 significant figures. Do not add unit in the answer.)
At high temperatures, A(s) decomposes to B(s) and C(g): 2A(s) - 3B(s) + C(g) When the rate of formation of B(s) is 7,169 M/s, the rate of decomposition of A(s) is M/s. (Answer should be in 3 significant figures. Do not add unit in the answer.)
4) At elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N2O3(g) - ANO, (2) + O2(g) Write the general rate expression using all chemical species: 5) Ar elevated temperatures, dinitrogen pentoxide decomposes to nitrogen dioxide and oxygen: 2N,Os(8) ANO, (g) + O, (g) When the rate of formation of NO, is 5.5 x 10-M/s, the rate of decomposition of No, is M/s. 6) . A[NH 1 = a[Nal = +2H2] = + Write the balanced equation for a...
For the reaction: 2A + 3B ---> 3D, if the rate of formation of D is 0.00645 M/s, determine the rate of disappearance of A: a. 0.00646 M/s b. 0.0194 M/s c. 0.00968 M/s d. 0.00430 M/s e. 0.00323 M/s
quick!!!!!!
Given the reaction at 300K: 2A(g) = 3B(g) + C(g) Kc = 5.5 x 10-5. If 12.0 moles of A is added to a 3.0L container (hint, you need molarity not moles in your ICE table), what will the concentration of A be at equilibrium? Neglect x for this problem. Report your answer to 2 significant figures. Answer: 3.8
9. At high temperatures, dinitrogen oxide gas decomposes to nitrogen according to the following equation: 2N20(g) 2N2(g) + 02(g) The following data are obtained in an experiment: and oxygen gases, Time (hr) 0 0.5 N-O 0.100 0.0934 0.0873 0.0815 0.0762 0.0665 0.0442 1.5 a) By plotting the data (on your own graph paper), show that the reaction is first-order. b) From the graph, determine k. c) Using k, find the time it takes to decrease the concentration to 0.0100 M
The reaction 2A + 3B → C is first order with respect to A and B. When the initial concentrations are [A] 1.55 x 10 2 M and [B] 2.11 × 10-3 M, the rate is 2.65 x 10 4 M. Calculate the rate constant or the reaction. Enter your answer in scientific notation. 10 O M ● M-1 M1.s1
please answer 9a,b,c,d
9. For the following reactions, predict whether they will tend to be spontaneous at high, low, ali temperatures, or non-spontaneous at any temperature (10 points) a) 2A(g) + 3B(9) C(g) + D(1), AH < 0 b) A() + B() (1) + D(s) AH > 0 c) A(s) + B(1) ► 20(1), AH < 0 d) 2A(s) B(s) + C(I), AH > 0
22 A) For the reaction
2A(g)+3B(g)⇌C(g)
Kc = 40.0 at a temperature of 165 ∘C∘
Calculate the value of Kp
22 B) For the reaction
X(g)+2Y(g)⇌2Z(g)
Kp= 1.87×10−2 at a temperature of 67 ∘C
Calculate the value of Kc
Part A For the reaction 2A(g) + 3B(g) = C(g) Kc = 40.0 at a temperature of 165 °C. Calculate the value of Kp. Express your answer numerically. View Available Hint(s) | ΑΣφ ? Submit Part B For the reaction X(g)...
Consider the equilibrium reaction: 2A (aq) + 3B (aq) <--> C (aq) (in my notation <--> means equilibrium arrows) Initially A is present at 6.00 M and B is present at 7.00 M. Also, initially there is no C present. At equilibrium B is present at 1.00 M. What is the Kc for this reaction? ( report your answer to 3 significant figures)