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Be sure to answer all parts. The thermal decomposition of phosphine (PH3) into phosphorus and molecular...
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
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
9. The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.50 × 10−3M, how long will it take for [A]t = 3.10 × 10−3M? ______ min (b) Calculate the half-life of the reaction. _______ min 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...
8. Consider the reaction: A → B The rate of the reaction is 1.6 × 10−2 M/s when the concentration of A is 0.35 M. Calculate the rate constant if the reaction is first order in A. Enter only the numerical value for the rate constant in the answer box. 9. The reaction 2A → B is second order with a rate constant of 51.0/M·min at 24°C. (a) Starting with [A]0 = 9.50 × 10−3M, how long will it take...
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 decomposition of phosphine forms phosphorus and hydrogen in the following reaction: 4PH3(g)--> P4(g)+6H2(g) A. express the rate with respect to each of the reactants and oroducts. B. if the instantaneous rate with respect to PH3 is 0.34 M s^-1, what is the instantaneous rate of the reaction? use rate laws not calculus please.
5. Phosphine (PH3) decomposes into phosphorus and molecular hydrogen: 4PH3(9) - P4(9) + 6H2(9) Experiments show that this is a first-order reaction, with a rate constant of 0.0173 s at 650°C. Identify each of the following statements about this reaction as true or false. (Use the drop-down menu and select "True" or "False" for each. You must get all 4 correct.) The rate constant would be smaller than 0.0173 sat 550°C. The reaction PH3 - PH2 + H might be...
Be sure to answer all parts. Consider the reaction 4PH3(g) → P4(g) + 6H2(g) Suppose that, at a particular moment during the reaction, molecular hydrogen is being formed at rate of 0.226 M/s. (a) At what rate is P4 changing? M/s (b) At what rate is PH3 changing? M/sF
Be sure to answer all parts. Consider the reaction 4PH3(g) →P4(g) + 6H2(g) At a particular point during the reaction, molecular hydrogen is being formed at the rate of 0.143 M/s. (a) At what rate is P4 being produced? M/s (b) At what rate is PH3 being consumed? M/s
How many grams of phosphine (PH3) can form when 35.0 g of phosphorus and 96.2 L of hydrogen gas react at STP? P4(s) + H2(g) → PH3(g) (Unbalanced) ....... g PH3