(a) Select all of the correct statements about reaction rates from the choices below.

The lower the rate of a reaction the longer it takes to reach completion.


A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant.


The rate of a fast step has more effect on the overall reaction rate than the rate of a slow step.


Solid catalysts increase reaction rates as their surface areas increase.


Slow reactions can be speeded up by raising the temperature.


Reactions involving very unstable combinations of chemicals have small rate constants.


Reaction rates always increase as masses of solid reactants increase.

2.90 moles of an ideal gas with Cv,m = 3R/2 undergoes the transformations described in the following list from an initial state described by T=310. K and P = 1.00 bar.

Part 1) The gas is heated to 725K at a constant external pressure of 1.00 bar. calculate q, w, delta U, delta H and delta S for this process.

Part 2) The gas is heated to 725 K at a constant volume corresponding to the initial volume. calculate q, w, delta U, delta H, delta S for this process

Part 3) the gas undergoes a reversible isothermal expansion at 310.K until the pressure is one third of its initial value. calculate q, w, delta U, delta H, delta S for this process

Balance the following reactions in acidic conditions. show all steps.

A). Mno4^-1 + C2O4^-2 --------- MnO2 + CO2

B). Br2 --------- Br^-1 + BrO^-1

C). Cu + NO3^-1 ---------- Cu^+2 + NO

D). MnO4^-1 + S^-2 --------- MnO2 + S

A mixture of 1.71 moles of B and 1.23 moles of C is placed in a 1.00 liter container at a given temperature and allowed to reach equilibrium according to the following equation. Calculate [A] present at equilibrium. Calculate [A] with 3 significant figures, exponential notation, and no units.

2A <----> B + C     K_c= 3

What is the vapor pressure of a solution made by adding 25.0 g of glucose, C6H12O6 (molar mass = 180. g/mol) to 145 g of water and heating the solution to 60 °C? The vapor pressure of pure water at 60 °C is 149 torr. The vapor pressure of pure glucose at 60 °C is negligible.

(a) 2.53 torr

(b) 127 torr

(c) 143 torr

(d) 146 torr

Consider the titration of a 21.0 −mL sample of 0.110 M HC2H3O2 with 0.125 M NaOH. Determine the pH after adding 6.00 mL of base beyond the equivalence point.

Calculate the equilibrium concentrations of N2O4 and NO2 at 25 degrees celcius in a vessel that contains an initial N2O4 concentration of 0.0500M. The equilibrium constant Kc for the reaction N2O4 (g) (equilibrium arrows here) 2NO2(g) is 4.64 x 10-3 at 25 degrees Celcius.

4.60 mol of solid A was placed in a sealed 1.00-L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.20 M, where it remained constant.

A (s) <---> B (g) + C (g)

Then, the container volume was doubled and equilibrium was re-established. How many moles of A remain?

Please break down the steps so I can see how to solve. Thank you!

Urea (CH4N2O) is a common fertilizer that can be synthesized by the reaction of ammonia (NH3) with carbon dioxide as follows:

2NH3(aq)+CO2(aq)→CH4N2O(aq)+H2O(l)

In an industrial synthesis of urea, a chemist combines 129.2 kg of ammonia with 211.4 kg of carbon dioxide and obtains 180.1 kg of urea.

1).Determine the theoretical yield of urea

2).Determine the percent yield for the reaction.

Write the net ionic equations that occur in the following cells:

1. Pb/Pb²⁺ // Ag⁺/Ag

2. Zn/Zn²⁺ // Pb²⁺/Pb

3. Al/Al³⁺ // Cd²⁺/Cd

Part B: An ideal gaseous reaction (which is a hypothetical gaseous reaction that conforms to the laws governing gas behavior) occurs at a constant pressure of 45.0 atm and releases 70.4 kJ of heat. Before the reaction, the volume of the system was 9.00 L . After the reaction, the volume of the system was 3.00 L .

Calculate the total internal energy change, ΔU, in kilojoules.

Part C:

An ideal gas (which is is a hypothetical gas that conforms to the laws governing gas behavior) confined to a container with a massless piston at the top. (Figure 2)  A massless wire is attached to the piston. When an external pressure of 2.00 atm is applied to the wire, the gas compresses from 5.40 to 2.70 L . When the external pressure is increased to 2.50 atm, the gas further compresses from 2.70 to 2.16 L .

In a separate experiment with the same initial conditions, a pressure of 2.50 atm was applied to the ideal gas, decreasing its volume from 5.40 to 2.16 L in one step.

If the final temperature was the same for both processes, what is the difference between q for the two-step process and q for the one-step process in joules?

A battery can provide a current of 3.4 A at 2.2 V for 1.5 hr. How much energy (in kj) is produced?

1. What effect does the presence of metal cations have on the color of a solution containing EBT at pH 10

2. What effect does the presence of metal cations have on the color of solution containing EDTA at pH 10?

3. Which ligand, EBT or EDTA, should be used as an indicator for a metal complexation reaction? What metals could this indicator be used for? Why?

4. Which ligand, EBT or EDTA, has a greater affinity for metal cations? What observations support your answer?

5. The water hardness titration is performed by first adding EBT and pH 10 buffer to the water sample, and then titrating with EDTA solution. Assuming that the water sample has calcium cations, what will be the color of the solution before and after the endpoint is reached? What do you tihnk the color at exactly the endpoint volume will be?

For the following electrochemical cell Cu(s)|Cu2 (aq, 0.0155 M)||Ag (aq, 1.50 M)|Ag(s)

write the net cell equation. Phases are optional. Do not include the concentrations.

Calculate the following values at 25.0 °C using standard potentials as needed.

E cell #1:

E cell #2:

G rxn #1:

Grxn#2:

there will be 4 answers total!