Based off these compounds, which one is the most hazardous and why?

Methyl Benzoate

Acetanilide

Nitric Acid (70%)

Acetic acid

Sulfuric Acid (98%)

The stopcock connecting a 1.00 L bulb containing helium gas at a pressure of 554 torr, and a 1.00 L bulb containing krypton gas at a pressure of 504 torr, is opened and the gases are allowed to mix. Assuming that the temperature remains constant, the final pressure in the system is ____torr

The binding energy per nucleon for magnesium-27 is 1.326*10^-12 J/nucleon. Calculate the atomic mass of magnesium-27, in amu. You may assume that the mass of a nucleon is 1.008 amu. (1 kg = 6.022*10²⁶ amu)

Consider an amphoteric hydroxide, M(OH)2(s), where M is a generic metal. M(0H)2 yields M+2OH M(OH)2 +2OH yields (M(OH4)2- Ksp=3x10^-16 Kf= .05 Estimate the solubility of M(OH)2 in a solution buffered at pH = 7.0, 10.0, and 14.0.

1. How could you distinguish between the following pairs using hydrogen NMR?
   1. cyclohexane and benzene
   2. butane and 2-methylpropane
   3. butyne and 1,3-dimethylbutane
   4. ethanol and dimethyl ether
   5. How could you distinguish between the pairs of compounds in question 1 using carbon NMR?

Draw structural formulas for all possible isomers having the following molecular formulas:

a. C₄H₁₀

b. C₂HBr₃

c. C₃H₆O

d. C₃H₄

Please explain also if you can. Thanks!

The reversible chemical reaction

A+B?C+D

has the following equilibrium constant:

Kc=[C][D][A][B]=3.4

Part A

Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?

Part B

What is the final concentration of D at equilibrium if the initial concentrations are[A] = 1.00M and [B] = 2.00M ?

What is the reaction A(g) + B(g) + C(g)------------> D(g) Experiment Initial [A] (mol/L) Initial [B] (mol/L) Initial [C] (mol/L) Initial rate (M/s) 1 0.0500 0.0500 0.0100 6.25*^(-3) 2 0.1000 0.0500 0.0100 1.25*^(-2) 3 0.1000 0.1000 0.0100 5*10^(-2) 4 0.0500 0.0500 0.0200 6.25*10^(-3)

1) What is the order with respect to each reactant?

2) Write the rate law

3) Calculate K (using the data from experiment 1)

Consider the titration of 50.0 mL of 0.0500 M C₂H₅NH₂ (a weak base; K_b = 0.000640) with 0.100 M HIO₄. Calculate the pH after the following volumes of titrant have been added:

3.00 g of potassium hydroxide (KOH) pellets are put into a constant-pressure calorimeter containing 250 mL of water. The initial temperature of the water is 22.3°C. The mixture is then stirred until all of the KOH is dissolved. The final temperature of the solution is measured and recorded as 29.7°C. Calculate the heat of solution for potassium hydroxide (ΔH_soln). The specific heat capacity of the solution may be assumed to be the same as that of water since this is a dilute solution. Assume no heat loss from the calorimeter.

What mass of KOH do you need to dissolve to reach a final temperature of  38 °C?

A sample of a substance with the empirical formula XBr2 weighs 0.5210 g. When it is dissolved in water and all its bromine is converted to insoluble AgBr by addition of an excess of silver nitrate, the mass of the resulting AgBr is found to be 0.6586 g. The chemical reaction is XBr2 + 2 AgNO32AgBr + X(NO3)2

(a) Calculate the formula mass of XBr2. Formula mass XBr2 = g mol-1

(b) Calculate the atomic mass of X. Atomic mass X = g mol-1

A beaker with 105 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 7.40 mL of a 0.430 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.

Express your answer numerically to two decimal places. Use a minus ( − ) sign if the pH has decreased.