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The rate law for the decomposition of phosphine (PHs) is APH, - kPH , Rate At...
can I please get help with this question. thanks 70) The thermal decomposition of phosphine (PHs)...
can I please get help with this question. thanks
70) The thermal decomposition of phosphine (PHs) into phosphorus and molecular hydrogen is a first-order reaction: 4PH)(g)-→ P,(g) + 6H2(g) The half-life of the reaction is 30.0 s at 682°C. Calculate (a) the first-order rate constant for the reaction and (b) the time required for 85 percent of the phosphine to decompose.
The rate law for the decomposition of PH3 is, R = -d[PH3]/dt = k[PH3]. It takes...
The rate law for the decomposition of PH3 is, R = -d[PH3]/dt = k[PH3]. It takes 120 s for the concentration of 0.84 M PH3 to decrease to 0.21 M. How much time is required for 1.5 M PH3 to decrease to 0.56 M?
The rate law for the decomposition of PH3 is, R = -d[PH3]/dt = k[PH3]. It takes...
The rate law for the decomposition of PH3 is, R = -d[PH3]/dt = k[PH3]. It takes 120 s for the concentration of 0.84 M PH3 to decrease to 0.21 M. How much time is required for 1.5 M PH3 to decrease to 0.56 M?
For problem #3 and 4, a. b. C. Calculate the rate constant. Calculate half life Calculate...
For problem #3 and 4, a. b. C. Calculate the rate constant. Calculate half life Calculate the time it takes for the concentration to go down to 75% of its original value. 3. The rate law for the decomposition of phosphine (PH3) is: Rate k [PH3] It takes 120. S for 1.00 M PH3 to go down to 0.250 M
The gas phase decomposition of phosphine at 120 °C PH3(g) 1/4 P_(g) + 3/2 H2(e) is...
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
Be sure to answer all parts. The thermal decomposition of phosphine (PH3) into phosphorus and molecular...
Be sure to answer all parts.The thermal decomposition of phosphine \(\left(\mathrm{PH}_{3}\right)\) into phosphorus and molecular hydrogen is a first-order reaction:\(4 \mathrm{PH}_{3}(g) \rightarrow \mathrm{P}_{4}(g)+6 \mathrm{H}_{2}(g)\)The half-life of the reaction is \(35.0 \mathrm{~s}\) at \(680^{\circ} \mathrm{C}\)Calcnlate the first-order rate constant for the reaction:_______s-1Calculate the time required for 95.0 percent of the phosphine to decompose:_______Col
Work set 3 The rate of sucrose's decomposition is given as rate of sucrose decomposition =...
Work set 3 The rate of sucrose's decomposition is given as rate of sucrose decomposition = k[sucrose] If k = 0.21/hr and the initial concentration of sucrose is 0.010 M, determine how much time must pass for the concentration (M) of sucrose to decrease by 90.0%.
The reaction B ➔ products follows the rate law Rate = k [B]2. If the initial...
The reaction B ➔ products follows the rate law Rate = k [B]2. If the initial concentration of B is 0.400 M, it requires 100 seconds for [B] to fall to 0.200 M. The additional reaction time (in seconds) that is required for [B] to reach 0.100 M is A. 125 B. 175 C. 100 D. 150 E. 200
Considering the rate law expression for decomposition, if the concentration of ammonia was increased 4 fold...
Considering the rate law expression for decomposition, if the concentration of ammonia was increased 4 fold (4 times), how many times will the reaction rate increase or decrease? Consider the rate law expression for synthesis and presume the concentration of H2 to be constant. If the concentration of nitrogen was increased 2 fold (2 times), how many times will the reaction rate increase or decrease?
The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0...
The rate law for the decomposition of N2O5 is rate = k[N2O5] If k = 1.0 x 10-5 s-1, what is the reaction rate when the N2O5 concentration is 0.0091 mol L-1? 2.The decomposition of acetaldehyde, CH3CHO, was determined to be a second order reaction with a rate constant of 0.0771 M-1 s-1. If the initial concentration of acetaldehyde is 0.301 M , what will the concentration be after selected reaction times? a. What will the CH3CHO concentration be after...
can I please get help with this question. thanks
70) The thermal decomposition of phosphine (PHs) into phosphorus and molecular hydrogen is a first-order reaction: 4PH)(g)-→ P,(g) + 6H2(g) The half-life of the reaction is 30.0 s at 682°C. Calculate (a) the first-order rate constant for the reaction and (b) the time required for 85 percent of the phosphine to decompose.
For problem #3 and 4, a. b. C. Calculate the rate constant. Calculate half life Calculate the time it takes for the concentration to go down to 75% of its original value. 3. The rate law for the decomposition of phosphine (PH3) is: Rate k [PH3] It takes 120. S for 1.00 M PH3 to go down to 0.250 M
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
Work set 3 The rate of sucrose's decomposition is given as rate of sucrose decomposition = k[sucrose] If k = 0.21/hr and the initial concentration of sucrose is 0.010 M, determine how much time must pass for the concentration (M) of sucrose to decrease by 90.0%.
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