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Trees in cold climates may be subjected to temperatures as low as -60 C. Estimate the concentration of an aqueous solution in the body of the tree that would remain unfrozen at this temperature. Is this a reasonable concentration? Comment on your result.
How many moles of oxygen atoms are combined with 4.20 moles of chlorine atoms in Cl2O7?
The reaction: 2 HI → H2 + I2, is second order and the rate constant at 800 K is 9.70 × 10-2 M-1 s-1. How long will it take for 8.00 × 10-2 mol/L of HI to decrease to one-fourth of its initial concentration.
2.00 L of H2 at a pressure of 368 torr and 1.00 L of N2 at an unknown pressure. If the total pressure in the flasks is 336 torr after the stopcock is opened.
A certain type of sugar dissolves in water, but the solution created does not conduct electricity. Therefore, the sugar does not form ions when dissolved in solution.
Determine the partial pressure of each gas in a mixture of gases using Dalton's law of partial pressures
What do you expect will happen to the position of this equilibrium when the total pressure of the gases in the reaction mixture is doubled by injecting some argon (Ar) while maintaining the temperature constant.
what we observed that 1.00 mole Hydrogen, 1.00 mol Iodine and 1.00 mole hydrogen iodide are introduced into a container of capacity 1.00-L. compute the concentrations of each species if equilibrium is reached?
Important information about Calculation, A person ate 0.50 pound of cheese (an energy intake of 4000kJ). Suppose that none of the energy was stored in the body
A chemist wants to make 5.5L of a 0.280M CaCl2 solution.What mass of CaCl2 (in g ) should the chemist use
if the density of mercury is 13.6g/cm3, what will be the volume of 300g of mercury ?
Define internal energy and enthalpy. What is the difference between the two? List the following gases in order of increasing root-mean-square speed, all at the same temperature: H2, He, O2, Ne
What volume, in liters, of O2 at 35°C and 1.19 atm can be produced from the decomposition of 10.0 g KNO3? 2 KNO3(s) → 2 KNO2(s) + O2(g)
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