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2000°C the equilibrium constant for the reaction is Kc = 2.4 103. 2 NO(g) N2(g) + O2(g) If the initial concentration of NO is 0.150 M, what are the equilibrium concentrations of NO, N2, and O2?
Metal X was plated from a solution containing cations of X. The passage of 48.25 C deposited 31 mg of X on the cathode. What is the mass of X (in grams) per mole of electrons.
At 25C, H2O2 decomposes according to the following equation. 2H2O2(aq) => 2H2O (l) + O2(g) .55V
What is the percentage protonation of the solute and Calculate the pH of the solute in an aqueous solution of 0.611 M Aqueous solution of Ammonia
Suppose 10.0 g of CH4 is used in a reaction that can theoretically produce 95.8 g of CCl4. What is the percent yield of CCl4 if the reaction produces only 80.0 g of CCl4.
A 5.0×101 sample of water absorbs 355 of heat.If the water was initially at 25.9, what is its final temperature.
Suppose you have a sample of sodium weighing 11.42 g. How many atoms of sodium are present in the sample.
Calculate the molar concentration of OH- ions in a 7.5×10^-2 M solution of ethylamine C2H5NH2(Kb = 6.4x10^-4).
2C4H10 + 13O2 → 8CO2 + 10H2O The equation shows the combustion of butane (C4H10). How many moles of water can be produced by 12.5 moles of C4H10 with excess oxygen.
At 25 oC the solubility of copper(II) iodate is 3.27 x 10-3 mol/L. Calculate the value of Ksp
Concentrated HCl is 36.5% HCl by mass and has a density of 1.18 g/mL.What is the molality?What is the molarity?
what is the maximum amount of P4S10(444.545 g/mol) which could be formed from 17.12 g of P4 (123.895 g/mol) and 0.137 mol of S8 (256.52 g/mol).
A gas was enclosed in a rigid-walled container. The initial temperature and pressure were 52°C and 0.55 atm, respectively. If the final pressure were 2.41 atm.
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