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Explain why light intensity is dependent on the distance the detector is from the light source. Describe the mathematical relationship. Explain why all comparative measurments for this experiment should be made with the optical cable the same distance from the light source.
Assume equilibrium with the calcium carbonate in the sediment and calculate the concentration of calcium ion (in mg/L -1) in the water (25C).
What volume of gaseous chlorine at STP would you need to obtain a 250.0 g sample of gas
What is the pH of a propanoic acid - propanoate buffer that is 0.25M in CH3CH2COONa and 0.15M with respect to CH3CH2COOH.
Predict the rate of change in the concentration of N2O over this time interval. In other words, what is dt [N2O]/ dt?
A mass of 1.37 g of an unknown gas is introduced into an evacuated 1.70 L flask If the pressure in the flask is 0.814 atm at 98 degrees C, which of the following gases might be in the flask?
Calculate the pH at the equivalence point for the titration of 0.240 M methylamine
What would be the value of the change in concentration of C10H12/change in time during the same period of time? Explain why a catalyst for a forward reaction must also be a catalyst for the reverse reaction. Include an energy level diagram
A 0.1000 m aqueous solution of a weak acid, HA, is 1.5% ionized. At what temperature does it freeze? Kf for water = 1.86°C/m.
Assume that sucrose is a molecular solid and does not ionize when it dissolves in water. Kf values are given here.
A sample of nitrogen gas is contained in a piston with a freely moving cylinder. At0?C, the volume of the gas is 248 mL. To what temperature must the gas be heated to occupy a volume of 479mL.
What is the enthalpy change for converting 1.00 mol of ice at -50.0°C to water at 70.0°C? The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K and 1.84 J/g-K respectively. For H2O, Hfus = 6.01 kJ/mol, and Hvap= 40.67 kJ/mol.
Use the appropriate standard reduction potentials to calculate the value
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