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A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of copper in a 1.0 M copper(II) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C.
What mass of calcium chloride is dissolved in 100. mL of a 1.20 M solution of calcium chloride
What is the internal energy of an ensemble of 1 mole of particles having two non-degenerate electronic energy levels separated by 1000cm^-1 at 1310K.
A sample of sodium reacts completely with 0.568 (kg) of chlorine, forming 936 (g) of sodium chloride. What mass of sodium reacted
what conditions does the rate equation reduce to second-order kinetics in NO and first kinetics in O2
A 1.30 M solution of citric acid (H3C6H5O7) in water has a density of 1.10 g/cm3. Calculate the mass percent, molality, mole fraction, and normality of the citric acid. Citric acid has three acidic protons.
Consider a situation in which 211g of P4 are exposed to 240g of O2. What is the maximum amount of P2O5 that can theoretically be made from 211g of P4 and excess oxygen?
For the reaction: N2(g) + 2 O2(g) ?? 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is twice the concentration of O2 gas
A mixture of 70 mole% butane and 30 mole % hyrdrogen is burned with excess air. Fractional conversion of 85% of the butane and 90% of the hydrogen are achieved
Are necessary to completely neutralize a solution in which 60.0g of NaOH have been dissolved
Write the rate law for this version of the iodine clock reaction. Could the rate law have been predicted using the coefficients in the balanced equation? Explain
Which of the following compounds would you expect to be ionic?
Describe what is meant by an amphoteric species. Write the equation for the self ionization of water and know the ion product constant expression for water and its value at 25 degrees.
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