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 6.40 to 3.20 LL . When the external pressure is increased to 2.50 atmatm, the gas further compresses from 3.20 to 2.56 LL .

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 6.40 to 2.56 LL 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?

Express your answer with the appropriate units.

A buffer solution contains 0.424 M ammonium chloride and 0.235 M ammonia.  

If 0.0297 moles of potassium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ?  
(Assume that the volume change does not change upon adding potassium hydroxide)

pH =

A buffer solution contains 0.382 M nitrous acid and 0.466 M potassium nitrite.  

If 0.0176 moles of hydrobromic acid are added to 150. mL of this buffer, what is the pH of the resulting solution ?  
(Assume that the volume change does not change upon adding hydrobromic acid)

pH =

A buffer solution contains 0.463 M KH₂PO₄ and 0.305 M Na₂HPO₄.  

If 0.0180 moles of sodium hydroxide are added to 150. mL of this buffer, what is the pH of the resulting solution ?  
(Assume that the volume does not change upon adding sodium hydroxide)

pH =

The equilibrium constant, K_c, for the following reaction is 1.80×10^-2 at 698 K.

2HI(g) -->H₂(g) + I₂(g)

Calculate the equilibrium concentrations of reactant and products when 0.257 moles of HI are introduced into a 1.00 L vessel at 698 K.

The equilibrium constant, K_c, for the following reaction is 83.3 at 500 K.

PCl₃(g) + Cl₂(g) -->PCl₅(g)

Calculate the equilibrium concentrations of reactant and products when 0.420 moles of PCl₃ and 0.420 moles of Cl₂ are introduced into a 1.00 L vessel at 500 K.

Draw the Sn1 intermediate and Sn2 transitions state for both ethyl-2-chloroacetate and benzyl bromide (α-bromotoluene). Use these structures to explain the differences in reactivity between these two compounds.

1. Some special GC detectors, such NPD and FPD, are often used to analyzed nitrogen containing and phosphorus containing pesticides, respectively, because these detectors have higher sensitivity than FID for the above-mentioned chemicals (T or F);
2. UV spectra always give sharp peaks that reflect the maximal absorption of chromophores (T or F);

A buffer solution contains 0.350 M NaHSO3 and 0.387 M Na2SO3. Determine the pH change when 0.104 mol HNO3 is added to 1.00 L of the buffer.

pH change =

This is all the info that was given

1a) A 2.95 g sample of an unknown chlorofluorocarbon (an organic compound containing chlorine and fluorine) is decomposed and produces 581 mL of chlorine gas at a pressure of 752 mmHg and a temperature of 298 K. What is the percent by mass of chlorine in the chlorofluorocarbon?

1b) Calculate the density of Freon-11 (CFCl3) at 118 °C and 7.20 atm

Should the order of spots of molecules on the TLC be different when two different eluent solvents are used? Explain your answer?

Should the TLC spot of a compound move higher or lower or stay the same when compared to in a less polar eluent solvent system when a more polar eluent solvent system is used?

If you started with 0.100g of tetraphenylcyclopentadienone and 0.100g of diphenylacetylene and obtained 0.089 g of hexaphenylbenzene from the experiment. Calculate percent Yield of hexaphenylbenzene?

Tetraphenylcyclopentadienone MolarMass= 384.478g/mol

diphenylacetylene MolarMass = 178.24 g/mol

With work shown

1) How many moles of H2O will be produced if 6.80 x 1024 formula units of NH4NO3 are decomposed in the reaction given below?

NH4NO3 -------- N2O + 2H2O

2) Aspirin (C9H8O4) can be made in the laboratory by reacting salicylic acid (C7H6O3) with acetyl chloride (C2H3ClO).

C7H6O3 + C2H3ClO-------- C9H8O4 + HCl

What mass of HCl is produced by the complete reaction of 36.0 g of acetyl chloride?

3) Propane (C3H8) burns in oxygen to form CO2 and H2O according to the following equation. How many grams of O2 are required to burn 3.01 x 1023 propane molecules?

C3H8 + 5 O2-------3 CO2 + 4 H2O

distinguish between analytical concentration and equilibrium concentration.

1- why do we say "error is inevitable"?

2- please distinguish between precision and accuracy .

Order these elements from MOST to LEAST reactive and explain your reasoning.

Ag, Cu, Fe, H, Mg, Ni, Pb, Sn, Zn

Solid Investigation Question:

What is the identity of an unknown solid piece of metal?

Specific questions:

1. What are the observable physical properties of your sample?

2. If provided with a table of densities of metals, how might you use this information to identify your piece of metal?

a. Given that calculating a physical constant is more reliable using a graph with multiple measurements from multiple samples than using measurements from a single sample, how could you use a graph to determine density if you are provided metal pieces of various lengths. Please note that you are required to submit a graph for your micro-project. Your graph will need to have a title, axes labels and a trendline as well as trendline equation. i

. How would you determine volume?

ii. What would you plot in order to get a slope that gives you density?

iii. What is the density of your sample?

Solution Investigation Question:

What are some of the key characteristics of unknown sample of an aqueous solution containing an ionic compound?

Specific questions: 1. Given that the cation is from Group 1A, what is the identity of the group 1A metal ion in your solution?

2. Given that the ionic compound contains either chloride or hydroxide, how can you determine which? (Two pieces of evidence are required and one must be related to solubility rules)

3. What is the concentration of your solution? (Your unknown sample is known to be about 1 M, but you need to determine the concentration to 3 significant figures using titration. You should plan ahead so that you know approximately what volume of your sample you will need in order to use approximately 25 mL of 0.100 M sulfuric acid for the titration). I'm not sure how to answer either of these problems

A reaction between substances A and B has b been found to give the following data:

Using the above data, determine the order of the reaction with respect to A and B, the rate law, and calculate the specific rate constant.

Given the values of ΔH∘rxn, ΔS∘rxn, and T below, determine ΔSuniv.

Predict whether or not each reaction will be spontaneous.

ΔH∘rxn=− 118 kJ , ΔS∘rxn= 261 J/K , T= 294 K

ΔH∘rxn= 118 kJ , ΔS∘rxn=− 261 J/K , T= 294 K .

ΔH∘rxn=− 118 kJ , ΔS∘rxn=− 261 J/K , T= 565 K .

ΔSuniv = ??? (J/K)