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The decomposition of phosphine, PH3, follows first-order kinetics: 4 PH3(g) → P4(g) + 6 H2(g) Calculate...
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 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
1) 2) 3) 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 9.50 x 10-2 S-1 ? Temperature = ______ oC
The isomerization of methyl isocyanide, CH3NC - CH3CN, follows first-order kinetics. The half-lives were found to be 161 min at 199°C and 12.5 min at 230°C. Calculate the activation energy for this reaction. (R-8.314 J/mol K) 124 kJ/mol 6.17 x 10-3kJ/mol 78.2 kJ/mol 163 kJ/mol 31.4 kJ/mo
6. (a) The rate constant for the first-order decomposition of N2Os in the reaction, 2 N2Os(g)-4 NO(g)+0.(g), k-3x10-s at 25°C. What is the half-life of N20s? What will be the pressure, initially 500 bar, at 10 min after initiation of the reaction? (b) Knowing the activation energy of the above reaction is 100 kJ mor', calculate the required reaction temperature at which the reaction rate is doubled. (c) What is the conversion efficiency of N20s at 1 bar and 25...
please answer 4,5, and 6 Thermodynamics versus Kinetics: The activation energy for the synthesis of Nha(g) from H2(g) and Nz(g) in the absence of catalyst is high, E.= 325 kJ/mol. The rate of the reaction may be increased by carrying out the synthesis at a high temperature (-500 °C). 4. Build a potential energy diagram for the synthesis of ammonia. 5. Determine how many times faster the reaction is at 500 °C than at 25 °C. 6. Determine how many...