(1):
When a 1.48-g sample of solid ammonium nitrate dissolves in 56.4
g of water in a coffee-cup calorimeter (see above figure) the
temperature falls from 22.00 oC to 20.09 oC.
Calculate H in kJ/mol
NH4NO3 for the solution process.
NH4NO3(s)
NH4+(aq) +
NO3-(aq)
The specific heat of water is 4.18 J/g-K.
Hsolution
= __kJ/mol NH4NO3.
(2):
The reaction S2O82-(aq) + 3 I-(aq) 2 SO42-(aq) + I3-(aq) was studied at a certain temperature with the following results:
Experiment | [S2O82-(aq)] (M) | [I-(aq)] (M) | Rate (M/s) |
---|---|---|---|
1 | 0.0309 | 0.0309 | 5.99e-06 |
2 | 0.0309 | 0.0618 | 1.20e-05 |
3 | 0.0618 | 0.0309 | 1.20e-05 |
4 | 0.0618 | 0.0618 | 2.39e-05 |
(a) What is the rate law for this reaction?
Rate = k [S2O82-(aq)] [I-(aq)]Rate = k [S2O82-(aq)]2 [I-(aq)] Rate = k [S2O82-(aq)] [I-(aq)]2Rate = k [S2O82-(aq)]2 [I-(aq)]2Rate = k [S2O82-(aq)] [I-(aq)]3Rate = k [S2O82-(aq)]4 [I-(aq)]
(b) What is the value of the rate constant?
(c) What is the reaction rate when the concentration of
S2O82-(aq) is 0.0602 M
and that of I-(aq) is 0.0655 M if the
temperature is the same as that used to obtain the data shown
above?
__ M/s
(1): When a 1.48-g sample of solid ammonium nitrate dissolves in 56.4 g of water in...
Part 1.) A flask is charged with 0.110 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) B(g) The following data are collected. times (s) 0 40 80 120 160 moles of A 0.110 0.070 0.043 0.032 0.024 (a) Calculate the number of moles of B at each time in the table. 0 s __ mol 40 s __ mol 80 s __ mol 120 s __ mol 160 s __...
When a 5.26-g sample of solid ammonium nitrate dissolves in 52.5 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 24.00 oC to 17.20 oC. Calculate H in kJ/mol NH4NO3 for the solution process. NH4NO3(s) NH4+(aq) + NO3-(aq) The specific heat of water is 4.18 J/g-K. Hsolution = _________kJ/mol NH4NO3.
When a 6.07-g sample of solid lead(II) nitrate dissolves in 31.9 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 22.00 oC to 18.47 oC. Calculate H in kJ/mol Pb(NO3)2 for the solution process. Pb(NO3)2(s) Pb2+(aq) + 2 NO3-(aq) The specific heat of water is 4.18 J/g-K. Hsolution = ?kJ/mol Pb(NO3)2.
When a 3.13-g sample of liquid sulfuric acid dissolves in 33.6 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 22.00 oC to 41.81 oC. Calculate H in kJ/mol H2SO4 for the solution process. H2SO4(l) 2 H+(aq) + SO42-(aq) The specific heat of water is 4.18 J/g-K. Hsolution =____ kJ/mol H2SO4.
When a 7.46-g sample of solid sodium hydroxide dissolves in 36.9 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 24.00 oC to 68.26 oC. Calculate H in kJ/mol NaOH for the solution process. NaOH(s) Na+(aq) + OH-(aq) The specific heat of water is 4.18 J/g-K. Hsolution = . kJ/mol NaOH.
When a 5.12-g sample of solid sodium nitrate dissolves in 31.1 g of water in a coffee-cup calorimeter (see above figure) the temperature falls from 25.00 oC to 16.37 oC. Calculate H in kJ/mol NaNO3 for the solution process. NaNO3(s) Na+(aq) + NO3-(aq) The specific heat of water is 4.18 J/g-K. We were unable to transcribe this imageWe were unable to transcribe this imagethermometer stirrer coffee cups containing reaction mixture When a 5.12-g sample of solid sodium nitrate dissolves in...
When a 4.09-g sample of gaseous hydrogen bromide dissolves in 42.6 g of water in a coffee-cup calorimeter (see above figure) the temperature rises from 21.00 oC to 42.94 oC. Calculate deltaH in kJ/mol HBr for the solution process. HBr(g) H+(aq) + Br-(aq) The specific heat of water is 4.18 J/g-K. delta Hsolution = _____ kJ/mol HBr. I entered answers 77.27 and 84.81 and both were incorrect
When a 4.25 g sample of solid ammonium nitrate dissolves in 60.0 g of water in a coffee-cup calorimeter, the temperature drops from 22.0 degrees C to 16.9 degrees C. Calculate Delta H kJ/mol NH4NO3 for the solution process NH4NO3 ( s) yields NH4 (there is a plus sign above the four)(aq) + ^ + NO3(negative sign above the three) (aq) Assume that the specific heat of the solution is the same as that of pure water. Express your answer...
Part 1.) A certain reaction has Ho = -26.10 kJ and So = 15.60 J/K. (a) Is this reaction exothermic, endothermic or isothermic (neither)? This reaction is ---Select--- exothermic endothermic or isothermic . (b) Does this reaction lead to a decrease, an increase, or no change in the degree of disorder in the system? This reaction leads to ---Select--- a decrease, an increase, or no change in the disorder of the system. (c) Calculate Go for this reaction at 298 K. If...
7) The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) → 2SO42−(aq) + I3−(aq) From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S2O82−](M) [I−](M) Initial Rate [M/s] 1 0.0200 0.0960 7.60 × 10−4 2 0.0200 0.0480 3.80 × 10−4 3 0.0400 0.0480 7.60 × 10−4 (a) Which of the following equations represents the rate law for this reaction? A. rate = k[S2O82−][I−] . ...