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Write chemical equations which show what happens when carbondioxide is absorbed by sodium hydroxide and when barium chloride isadded to the solution. Use these equations to justify our method for estimating carbon dioxide concentration.
A sample in a 1.0 mm cell absorbs 75.0% of the incident light at 510 nm. If the solution is 0.075 M, its molar absorptivity (M-1 cm-1) is:
Draw the structure of the compound identified by the following simulated 1H and 13C NMR spectra.
The energy difference of 3.8 kJ/mol between gauche and anti butane corresponds to an equilibrium constant, Keq, of approximately 1.9. Calculate the percentage of each conformer at equilibrium.
A buffer contains 0.30 M acetic acid and 0.20 M sodium acetate. What is the pH of the buffer as prepared and after 0.030 mol/L of a strong acid or 0.030 mol/L of a strong base are added (Ka = 1.8 x 10-5).
Calculate the value of Delta G for the process- AgCl (s) Ag+(aq) + Cl-(aq) to yield a saturated solution at 298 K.
A bomb calorimeter whose components have a heat capacity of 6.66 kJ/°C is filled with 913 g of water. (The amount of water is not constant from experiment to experiment.
Mixtures of diastereomeric 1,3-dimethylcyclopentanes are formed on catalytic hydrogenation of all but one of the following. Which compound gives only a single stereoisomer of 1,3-methylcyclopentane
Hydrogen iodide decomposes according to the equation: 2HI(g) H2(g) + I2(g) Kc = 0.0156 at 400°C. A 0.57 mol sample of HI was injected into a 2.0 L reaction vessel held at 400°C. Calculate the concentration of HI at equilibrium.
write the formula of the complex ion formed between a. the ligand cl- and the copper ii ion with a coordination number
The first-order rate constant for the reaction of methyl chloride (CH3Cl) with water to produce methanol (CH3OH) and hydrochloric acid (HCl) is 3.32 10-10s-1 at 25°C. Calculate the rate constant at 38°C if the activation energy is 116 kJ/mol.
Calculate the electron affinity in kJ/mol for X in the hypothetical ionic compound MX from the information given below.
At 400 K, an equilibrium mixture of H2, I2, and HI consists of 0.015 mol H2, 0.012 mol I2, and 0.025 mol HI in a 4.50-L flask. What is the value of Kp for the following equilibrium? (R = 0.0821 L · atm/(K · mol))2HI(g) H2(g) + I2(g)
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