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Predict the change in energy (J/photon) that occurs when an electron moves from n = 2 to n = 1.
A certain quantity of a gas occupies 61.3 mL at 68 ?C. If the pressure remains constant, what would be the volume of the gas at 128 ?C?
Calculate the amount of work done against an atmospheric pressure of 1.00 atm when 500.0 g of zinc dissolves in excess acid at 30.0°C. Zn(s) + 2H+(aq) → Zn2+(aq) + H2(g)
a helium-filled weather balloon is launched from the ground where the pressure is 752 mmHg and the temperature is 21 degrees celsius. under these conditions its volume is 75.0 L.
a reaction takes place in which a gas is one of the products. The gas had a d=1.81 g/L at 1.00 atm and 23 degrees C. What is the molar mass and identity of the gas?
For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction?
Determine the number of moles of O2 produced by the decomposition of 213 g of NaClO3.
A chemist burns 160g of aluminum oxygen to produce aluminum oxide. She produces 260g of aluminum oxide. Write a balanced equation and calculate the theoretical and percent yield
What is the percent by mass of oxygen in a gaseous mixture whose molar composition is 0.500% CO2 and 99.500% air. The composition of air is 21% mole O2, 79% mole N2, and has an average molar mass of 29.0 g/mol.
The half-lives of different radioisotopes are given in the table below. If the initial amount of indium-117 is 8.4 g, how much indium-117 is left in the body after 86 minutes?
Ethanol normally boils at 78.4C. the boiling point elevation constant for ethanol is 1.22C/m. what is the boiling point of a 1.0 m solution
A mixture of three gases has a total pressure at 293K of 1380 mmHg. The mixture is analyzed and is found to contain 1.27 mol CO2, 3.04 mol CO, and 1.50 mol Ar. What is the partial pressure of Ar?
If the final tempurature of the combined water is 42.0 degrees C and the heat capacity of the calorimeter is 26.3 J/degrees C , calculate the mass of the water originally in the calorimeter
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