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methane flowing at 2 mol/min is adiabatically compressed from 300 K and 1 bar to 10 bar. What is the minimum work required? Use Departure Functions.
the 1H NMR spectrum contains a triplet at 1.08 ppm (3H), a singlet at 2.5 ppm (3H), and a quartet at 2.45 ppm (2h). the magnitudes of the splitting of both the quartet and triplet are identical. ded
A chemical reaction at equilibrium is heated, briefly, by holding it over a flame. The equilibrium is seen to shift toward the products. What can be said about the enthalpy and entropy of the reacti
There are two properties of a chemical system that determine whether it can happen spontaneously, if the pressure and temperature don't change. These properties are
If the pressure during the reaction stays CONSTANT (but the volume can change, like in a piston or balloon), which of these reactions do work on the surroundings
what is the ph of a Solution prepared by mixing 163.0 ml of 2.4×10?3 MHCl and 382.0 ml of 1.4×10?3 HClO4 (Assume that volumes are additive.)
If .050 moles of HA were dissolved in 1L of water, calculate the concentration of [HA], [H30+], and [A-] in the solution at equilibrium. What is the pH? Ka=7.94 x 10^-7, equivalence point ~ 9 mL, pH
Explain the oxidation reduction happening behind the reaction: 2 NH4NO3 (s) -> 2N2 (g) + O2 (g) + 4H2O (l)
The IR spectrum of HCN shows three absorption bands at 3312 cm-1, 2089cm-1, and 712 cm-1. Assuming HCN is linear, assign vibrations to the three absorption bands
The reagents available other than DI water are 3.0 M solutions of any acid or base that you may need. How would you go about preparing this buffer
Put the following substances in correct order of increasing boiling point: Ar, F2, H3COH, Ir, SO2.
Explain for which of the following species resonance is an important property: HONO, HONO2, N3-, NO2-, NO2.
The pH of rainwater in a polluted area was found to be 3.50. What is the H+ concentration
Calculate the solubility at 25 degrees Celsius in grams per liter of AgI in a solution that is 0.15 M in potassium iodide and 0.25M in ammonia. State any equilibrium constants you use.
A solution is created by adding 0.05 moles of H2CO3 (3.1 g, total mass) to 5-L of water, resulting in a pH of 4.2. Now, we add sodium hydroxide (NaOH, strong base) until the pH reaches 10. You can n
A solution is created by adding 0.05 moles of H2CO3 (3.1 g, total mass) to 5-L of water, resulting in a pH of 4.2. Now, we add sodium hydroxide (NaOH, strong base) until the pH reaches 7. You can ne
Calculate the equilibrium constant at 0c and at 50c(assuming enthalpies of formation are independent of temp)
A water sample is measured to have alkalinity of 130 mg/L as CaCO3 at pH=9.2, what are the concentrations of the three carbonate species
A solution is created by adding 0.05 moles of H2CO3 (3.1 g, total mass) to 5-L of water, resulting in a pH of 4.2. What is the alkalinity of this water (in meq/L)? Does the answer make sense, why or
A water at pH = 6.35 has HCO3- concentration of 2.2 mM. What is the alkalinity? Clearly specify your units
What is the equilibrium pH of the solution? Solve by graphical method (draw a log C -pH graph and label the pertinent info, show your charge balance for the equation)
at room temperature more of the collisions have sufficient energy to produce a reaction. the piece of zinc needs to be bigger at 4 deg c.
Consider the following reversible reaction. In a 1-liter container the following amounts are found in euilibrium at 400 deg C., 0.0536 mole N2, 0.599 mole H2, and 0.0437 mole NH3. Evaluate Kc = N2(g
Draw the major E2 reaction product formed when (1R,2S,4S)-2-chloro-4-methyl-1- (propan-2-yl)cyclohexane (shown below) reacts with hydroxide ion in DMSO.
Suppose you wished to control the PO43- concentration in a solution of phosphoric acid by controlling the pH of the solution. If you assume you know the H3PO4 concentration, what combined equation w