An unknown inorganic phosphate undergoes first-order dehydration in a drying oven. Initially, the excess water content is measured to be 2.20 mg. After 2.30 days the water content is reduced to 1.24 mg. After 4.30 days, water content is only 0.751 mg. Determine the half-life of hydration under these conditions. Give the answer to 3 significant figures

An unknown inorganic phosphate undergoes first-order dehydration in a drying oven. Initially, the excess water content is measured to be 2.20 mg. After 2.30 days the water content is reduced to 1.24 mg. After 4.30 days, water content is only 0.751 mg. Determine the half-life of hydration under these conditions. Give the answer to 3 significant figures

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 25QRT

See similar textbooks

Similar questions

Determine whether the following statements are true or false, and explain your answer in one sentence. a) The rate law for an overall reaction 2A (g) -> B (g) is: Rate = k[A]^2 b) The rate law for an elementary step 2A (g) -> B (g) is: Rate = k[A]^2 c) The rate of an overal reaction is the rate of the slowest elementary step within its mechanism.
Calculate the velocity of the reaction (M · s–1) of an α-amino group in a blood protein at 37°C if its concentration is 0.60 mM and the partial pressure of carbon dioxide is 40 torr. Use 2 significant figures and scientific notation (example: 1000 would be entered as 1.0e+3). The rate constant k for this reaction is 4950 M–1·s–1.
The enzyme urease increases the rate of urea hydrolysis at pH 8.0 and 20 °C by a factor of 1014. Suppose that a given quantity of urease can completely hydrolyze a given quantity of urea in 19 minutes at pH 8.0 and 20 °C. How long would it take for this amount of urea to be hydrolyzed in the absence of urease at the same temperature and pH in sterile conditions? Include two significant figures in your answer. timeuncatalyzed years * TOOLS x10
Consider the reaction a A(aq) → bB(aq) (1) Where a and b are stoichiometric coefficients for the balanced chemical reaction The average reaction rate r can be measured if the concentration change of the reagents or products is known: 1 ΔΙΑ 1 Δ r = and r = At b At a where A and B notate the concentration of A and B in solution, and A is always defined as the difference between "final" and "initial": A[4] = [A],2 - [4],1 and At = t2 – t . - A particular case of eq. (1) could be A(aq) → 2 B(aq) If the initial concentration of B is 0.2569 mol L1, and after 415.6 s it increases to 0.4633 mol L1, what is the rate of the reaction in mol L1s? mol L-1 s1. (Use scientific notation)
Time [Z] (hours) (mg/L) |160 2 |140 3 |130 6 100 8 80 10 |60 |12 40 Calculate k, the elimination rate constant, responsible for drug degradation (in mg/L*hr).
In aqueous solution buffered at a pH of 6.75 Penicillin G (molecular weight of 334.39 g/mole) undergoes hydrolysis via a pseudo first order reaction that has an activation energy of 77.3 kJ/mole and a pseudo first order rate constant of 1.58 x 10-7 s-1 at 30°C. The solubility of the sodium salt of Penicillin G is 25 mg/ml of water. One would expect the solubility of the sodium salt to be ____________ that of the Penicillin G. a. higher than b. the same as c. lower than
How do I mathematically express this reaction in terms of Qc
1 Rate constants for the first-order decomposition of acetonedicarboxylic acid CO(CH2COOH)2(aq) → CO(CH3)2(aq) + 2 CO2(g) acetonedicarboxylic acidacetone are k = 4.75 ×10–4 s–1 at 293 K and k = 1.63 ×10–3 at 303 K. What is the activation energy, Ea, for this reaction? Select one: a. 71KJ/mol b. 81KJ/mol c. 51KJ/mol d. 91kJ/mol
The equation for the iodination of acetone in acidic solution isCH3 COCH3(aq) + I2(aq) → CH3 COCH2(aq) + H+(aq) + I- (aq) The rate of the reaction is found to be dependent not only on the concentration of the reactants but also on the hydrogen ion centration. Hence the rate expression of this reaction is: rate = k [CH3COCH3]m [I2 ]n [H+]p The rate is obtained by the following the disappearance of iodine using starch as an indicator. The following data are obtained: [CH3COCH3] [H+] [I2] Initial Rate (mol/L.s) 0.80 0.20 0.001 4.2 x 10-6 1.6 0.20 0.001 8.2 x 10-6 0.80 0.40 0.001 8.7 x 10-6 0.80 0.20 0.0005 4.3 x 10-6 1. What is the order of the reaction with respect to each reactant? 2. Write the rate expression for the reaction.3. Calculate, K4. What is the rate of the reaction when [H+]= 0.933 M and [CH3COCH3]= 3[H+]= 10[I-] ?
If tripling the concentration of a single reactant R in a multi-reactant reaction (while leaving all other conditions unchanged) leads to a nine−fold increase in rate, it can be deduced
The rate law for the reaction A + B → C was found to be rate = k[A][B]. One experimental trial with the [A] = 0.26 M and (B] = 0.13 M had an initial rate of product formation of 0.36 M/s. What is the value of the rate constant for this reaction? Enter your answer as 0.0035 with no units. Use 2 significant digits. Answer:
A) Determine the freezing point of an aqueous solution created from 3.5 g of Na3PO4 added to 120.0 g of water. The molal freezing point depression constant of water is 1.86 °C/m. Report your answer to 2 significant figures in degrees celcius but do not type in the units. B) For the first order reaction 2X --> N + 3P, the half life is measured as 50 seconds. If the initial solution concentration is 3 M, how long must the reaction proceed to consume 30% of the original amount of X? Give your answer in seconds.