![The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction when N205] = 0.0270? Expr](http://img.homeworklib.com/questions/be9ba5b0-d070-11eb-b8b6-fdaf6c1f7363.png?x-oss-process=image/resize,w_560)
Homework Answers
![Decomposition of N, C 21,45 —>4NO2 + O2 date constant(K) -- 4B 2 X10-35Y Part-B rately)=K [N2O5] here. [N, Os] = 0.0270 M. r](http://img.homeworklib.com/questions/c0cfe730-d070-11eb-bede-9b483e7b812a.png?x-oss-process=image/resize,w_560)
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The decomposition of N2O5 in carbon tetrachloride proceeds as follows: What is the rate of reaction...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first...
The decomposition of N2O5 in carbon tetrachloride proceeds as follows: 2N2O5→4NO2+O2 The rate law is first order in N2O5. At 64*C the rate constant is 4.82 ×10^−3s^−1 The rate law is 4.82x10-3s-1 [N2O5] The rate of rxn when [N2O5]=2.40x10^-2 M is 1.16x10^-4 M/s What happens to the rate when the concentration of N2O5 is doubled? What about halved? The answers are NOT 9.64x10^-3 and 2.41x10^-3 M/s
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction: 2N2O5 (soln) →...
The decomposition of N2O5 in solution in carbon tetrachloride proceeds via the reaction: 2N2O5 (soln) → 4NO2 (soln) + O2 (soln) The reaction is first order and has a rate constant of 4.82 x 10-3 s-1 at 64 oC. The reaction is initiated with 0.058 mol in a 1.25 L vessel. What is the half-life of the reaction?
The following reaction is first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is
first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for
the reaction at a certain temperature is 0.053/s. You may want to
reference (Pages 593 - 598) Section 14.4 while completing this
problem. Part A Calculate the rate of the reaction when [N2O5]=
5.7×10−2 M. Express your answer using two significant figures. rate
= nothing M/s Request Answer Part B What would the rate of the
reaction be at the same concentration as in Part A if...
The following reaction is first order in N2O5N2O5: N2O5(g)→NO3(g)+NO2(g)N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at...
The following reaction is first order in N2O5N2O5: N2O5(g)→NO3(g)+NO2(g)N2O5(g)→NO3(g)+NO2(g) The rate constant for the reaction at a certain temperature is 0.053/s/s. Part A Calculate the rate of the reaction when [N2O5]=[N2O5]= 5.1×10−2 MM. Express your answer using two significant figures. rate= ______ M/s Part B What would the rate of the reaction be at the same concentration as in Part A if the reaction were second order? (Assume the same numerical value for the rate constant with the appropriate units.)...
< Problem Set #4 (ch 14) Exercise 14.50 - Enhanced - with Feedback The data below...
< Problem Set #4 (ch 14) Exercise 14.50 - Enhanced - with Feedback The data below show the concentration of N205 versus time for the following reaction: N2O5 (g) → NO3(g) + NO2(g) Time (s) [N2O5] (M) 1.000 0.822 0.677 25 50 0.557 0.458 0.377 100 125 150 175 200 0.310 0.255 0.210 Part B Determine the value of the rate constant. Express the rate constant to three significant figures VAZO + # O ? k = Submit Request Answer...
1A. The decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C N2O5 2 NO2...
1A. The decomposition of dinitrogen pentoxide in carbon
tetrachloride solution at 30 °C N2O5 2 NO2 + ½ O2 is first order in
N2O5 with a rate constant of 4.10×10-3 min-1. If the initial
concentration of N2O5 is 0.510 M, the concentration of N2O5 will be
M after 402 min h
1B. The gas phase decomposition of phosphine at 120 °C
PH3(g)1/4
P4(g) + 3/2 H2(g)
is first order in PH3
with a rate constant of 1.80×10-2
s-1.
If the...
Constants Periadic Table Part A The first-order rate conslant for the decomposition of N O 2N20s(8)4NO2(8)...
Constants Periadic Table Part A The first-order rate conslant for the decomposition of N O 2N20s(8)4NO2(8) +02(8) How many moles of N20s will remain after 5.0 min? Express the amount in moles to two significant digits. at 70 C is 6.82 x 10-3-1. Suppose we start with 2.20x10-2 mol of N2O (g) in a volume of 1.8L You may want to reference (Pages 587 - 592) Section 14.4 whille completing this problem mol Submit Request Answer Part B How many...
For the reaction shown, calculate how many moles of NO, form when each amount of reactant...
For the reaction shown, calculate how many moles of NO, form when each amount of reactant completely reacts. 2 N,Os(9) + 4NO2(g) + O2(9) Part C 4.75 x 10' mol N205 Express your answer using three significant figures. AXO O ? % 1.02 mol Submit Previous Answers Request Answer * Incorrect; Try Again; 5 attempts remaining Part D 1.008 x 10-mol N, O, Express your answer using four significant figures. V ASD - O ? mol Submit Request Answer
Need help with part B and C <Assignment 15 Chap 14: Determining Rate Laws Problem 14.30...
Need help with part B and
C
<Assignment 15 Chap 14: Determining Rate Laws Problem 14.30 - Enhanced - with Feedback ® 3014 ~ M Review | Constants Periodic Table Consider the following reaction: 2NO(g) + 2H2(g) →N2(g) + 2H2O(g). You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. If the rate constant for this reaction at 1000 K is 6.0 x 104 M-s-7, what is the reaction rate when (NO) = 2.80x10-2 M...
Part A Review ConstantsI Periodic Table How many moles of N2O, will remain after 7.0 min? The first-order rate constant...
Part A Review ConstantsI Periodic Table How many moles of N2O, will remain after 7.0 min? The first-order rate constant for the decomposition of N2 O Express the amount in moles to two significant digits. 2N2Os (g)+4NO2(g) +02(g) n1.6x10-3 mol at 70° C is 6.82 x 103 s-, Suppose we start with 2.80x102 mol of N2O5 (g) in a volume of 2.0 L You may want to reference (Page) Section 14.4 while completing this problem. Correct The rate of reaction...
The following reaction is
first order in N2O5: N2O5(g)→NO3(g)+NO2(g) The rate constant for
the reaction at a certain temperature is 0.053/s. You may want to
reference (Pages 593 - 598) Section 14.4 while completing this
problem. Part A Calculate the rate of the reaction when [N2O5]=
5.7×10−2 M. Express your answer using two significant figures. rate
= nothing M/s Request Answer Part B What would the rate of the
reaction be at the same concentration as in Part A if...
< Problem Set #4 (ch 14) Exercise 14.50 - Enhanced - with Feedback The data below show the concentration of N205 versus time for the following reaction: N2O5 (g) → NO3(g) + NO2(g) Time (s) [N2O5] (M) 1.000 0.822 0.677 25 50 0.557 0.458 0.377 100 125 150 175 200 0.310 0.255 0.210 Part B Determine the value of the rate constant. Express the rate constant to three significant figures VAZO + # O ? k = Submit Request Answer...
Constants Periadic Table Part A The first-order rate conslant for the decomposition of N O 2N20s(8)4NO2(8) +02(8) How many moles of N20s will remain after 5.0 min? Express the amount in moles to two significant digits. at 70 C is 6.82 x 10-3-1. Suppose we start with 2.20x10-2 mol of N2O (g) in a volume of 1.8L You may want to reference (Pages 587 - 592) Section 14.4 whille completing this problem mol Submit Request Answer Part B How many...
For the reaction shown, calculate how many moles of NO, form when each amount of reactant completely reacts. 2 N,Os(9) + 4NO2(g) + O2(9) Part C 4.75 x 10' mol N205 Express your answer using three significant figures. AXO O ? % 1.02 mol Submit Previous Answers Request Answer * Incorrect; Try Again; 5 attempts remaining Part D 1.008 x 10-mol N, O, Express your answer using four significant figures. V ASD - O ? mol Submit Request Answer
Need help with part B and
C
<Assignment 15 Chap 14: Determining Rate Laws Problem 14.30 - Enhanced - with Feedback ® 3014 ~ M Review | Constants Periodic Table Consider the following reaction: 2NO(g) + 2H2(g) →N2(g) + 2H2O(g). You may want to reference (Pages 576 - 581) Section 14.3 while completing this problem. If the rate constant for this reaction at 1000 K is 6.0 x 104 M-s-7, what is the reaction rate when (NO) = 2.80x10-2 M...
Part A Review ConstantsI Periodic Table How many moles of N2O, will remain after 7.0 min? The first-order rate constant for the decomposition of N2 O Express the amount in moles to two significant digits. 2N2Os (g)+4NO2(g) +02(g) n1.6x10-3 mol at 70° C is 6.82 x 103 s-, Suppose we start with 2.80x102 mol of N2O5 (g) in a volume of 2.0 L You may want to reference (Page) Section 14.4 while completing this problem. Correct The rate of reaction...
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