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The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate...
For the gas phase decomposition of phosphine at 120 °C 4 PH3(g)P4(g) + 6 H2(g) the average rate of disappearance of PH3 over the time period from t = 0 s to t = 27 s is found to be 2.63×10-4 M s-1. The average rate of formation of H2 over the same time period is________ M s-1.
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 initial concentration of PH3 is 5.86×10-2 M, the concentration of PH3 will be 1.43×10-2 M after s have passed.
10. The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first-order reaction: 4PH3(g) → P4(g) + 6H2(g) The half-life of the reaction is 35.0 s at 680°C. a) Calculate the first-order rate constant for the reaction: _______ s−1 b) Calculate the time required for 78.0 percent of the phosphine to decompose: ________ s
The following data are for the gas phase decomposition of phosphine at 120 °C. PH3(g) 1/4 P4(g) + 3/2 H2(g) [ PH3 ], M 4.94×10-2 2.47×10-2 1.24×10-2 6.20×10-3 time, s 0 25.8 51.6 77.4 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is__ s . (2) Based on these data, the rate constant for this order reaction is__ s -1
The gas phase decomposition of phosphine at 120 °C PH3(g) 1/4 P_(g) + 3/2 H2(e) is first order in PH, with a rate constant of 1.80x102;! If the initial concentration of PH, is 6.66x102 M, the concentration of PH, will be 1.09x10-2 M after s have passed
Consider the reaction 4 PH3(g) → P4(g) + 6 H2(g). If, in a certain experiment, over a specific time period, 0.0045 mole of PH3 is consumed in a 1.7-L container during each second of the reaction, what are the rates of production of P4 and H2 in this experiment? P4 mol L−1 s−1 H2 mol L−1 s−1
Phosphine, PH3, a reactive and poisonous compound, reacts with oxygen as follows: 4PH3(g) + 802(g) → P4010(s) + 6H20(9) If 15.0 g of phosphine reacts with sufficient oxygen, how many grams of P4010 will be formed? Multiple Choice o O 125 g o 3139 31.3g o О 500 x 102 g o О 18.9 g o 75.7 g 757 g
Question 1 P4 (s) + 6 H2(g) → 4 PH3(g) What are the correct mole ratios based on the chemical equation above? BLANK-1 mol P4 : BLANK-2 mol PH3 BLANK-3 mol H2 : BLANK-4 mol PH3 BLANK-5 mol P4: BLANK-6 mol H2 BLANK-1 Add your answer BLANK-2 Add your answer BLANK-3 Add your answer BLANK-4 Add your answer BLANK-5 Add your answer BLANK-6 Add your answer
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The decomposition of dinitrogen tetroxide to nitrogen dioxide at 400°C follows first-order kinetics with a rate constant of 3.84 X10-3-1. Starting with pure N204, how many minutes will it take for 38.0% to decompose? Suppose the surface-catalyzed hydrogenation reaction of an unsaturated hydrocarbon has a rate constant of 0.374 M/min. The reaction is observed to follow zero-order kinetics. If the initial concentration of the hydrocarbon is 2.90 M, what is the half-life of the reaction in seconds?...
The following gas-phase reaction follows first-order kinetics. CIO2F======> CIOF+O The activation energy of this reaction is 186 kJ/mol. The value of k at 322°C is 6.76 x 10-4 S-1 . a. What would be the value of k for this reaction at room temperature, 25°C? k = _____ S-1 b. At what temperature would this reaction have a k value of ? Temperature = ______ oC