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For the reaction A ? B, ?G = -60 kJ/mol. The reaction is started with 10 mmol of A. no B is initially present. After 24 hours, analysis reveals the presence of 0.2 mmol of B, 9.8 mmol of A. Which is the most likely explanation? a. A and B have reached equilibrium concentrations. b. Formation of B is thermodynamically unfavorable. c. The result described is impossible, given the fact that delta G is -60 kJ/mol. d. The activation energy for the reaction is very large; equilibrium has not been reached by 24 hours. e. An enzyme has shifted the equilibrium toward A.
What is the molarity of a nitric acid solution if 43.53 mL 0.1000 M KOH solution is needed to neutralize 20.00 mL of the acid solution
For a given reaction the following half-life and initial concentration data was collected. Use this data to determine the reaction's order and rate constant.
In coffee, how much would the boiling point (in C) of the water be raised by the addition of 0.2 g of caffeine (C8H10N4O2) to 5.0 L of water in making this so much coffee
What mass of potassium bromide residue remains if 500.0 mL of 0.200 M potassium bromide solution are evaporated to dryness?
Draw the most stable chair conformation for (1S,3S)-1-chloro-3-ethylcyclohexane. Please explain your answer.
what is the temperature of the air inside of the tire when the pressure increases to 29 psi? Assume tire volume is constant.
Using the half-reaction method, balance the following oxidation-reduction reaction which occurs in acidic solution. Be sure to show the each step in balancing both half-reactions
When runners or other athletes practice at high altitudes pressure is reduced. What then will be the effect on the [O2] in their blood? Why does this produce a lightheaded feeling?
What is the net ionic equation for this reaction occurring in water: Potassium sulfate and barium chloride are mixed to form potassium
what is the oxidation number of the specified element in each compound or polyatomic ion: a)C in ZnCO3 b)Fe i Fe(NO3)2 c)Cl in ClF4^- d)S in S2O3^2-
Consider the titration of 100.0 mL of 0.100 M H2NNH2 (Kb = 3.0 10-6) by 0.200 M HNO3. Calculate the pH of the resulting solution after the 20.0 mL of HNO3 have been added.
Write the balanced chemical equation for the reaction of aqueous phosphoric acid with aqueous sodium hydroxide (NaOH is being titrated). Then calculate the volume of .200 M H3PO4 could be neutralized using 50.00 ml of your diluted NaOH
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