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Given the following Delta H°298 values in kcal/mol , where "gr" stands for graphite, find Delta f H°298 of Fe(s) and Fe2O3(s) Fe2O3(s) + 3C (gr) --> 2Fe(s) + 3CO(g) 117 FeO(s) + C(gr) --&
Calculate individual concentrations in an unknown mixture. Calculate the individual concentrations of C and of D in the following unknown mixture: Compound C: Absorbance at 365nm = 0.150 Absorbance
In the lab using conc. HCL and heat, if the solubities of reactant and product were reversed , how would the isomerization be followed. How would one knows when it is complete
The system then re-equilibrates. The appropriate chemical equation is PCl3(g)+Cl2(g)<---->PCl5(g) Calculate the new partial pressures of PCl3, Cl2, and PCl5 after equilibrium is reestablished.
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g) is injected into the mixture, and the total p
At equilibrium, the concentrations in this system were found to be [N2]=[O2]=0.100 M and [NO]=0.400 M. N2(g)+O2(g)<---->2NO(g) If more NO is added, bringing its concentration to 0.700 M, what
At a certain temperature, the Kp for the decompositon of H2S is 0.800. H2S(g0<----->H2(g)+S(g) Initally, only H2S is present at a pressure of 0.239 atm in a closed container. What is the total
A 0.291 mol sample of PCl5(g) is injected into an empty 4.35 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.
A(aq)<----->2B(aq) Kc-7.97e-6 at 500K If a 3.40 M sample of A is heated to 500 K, what is the concentration of B at equilibrium
Carbon disulfide is prepared by heating sulfur and charcoal. The chemical equation is S2(g)+C(s)<----> CS2(g) Kc=9.40 at 900K How many grams of CS2(g) can be prepared by heating 16.4 moles of
At a certain temperature, the equilibrium constant, Kc, for this reaction is 53.3. H2(g)+I2(g)<---->2HI(g) Kc=53.3 At this temperature, 0.800 mol of H2 and 0.800 mol of I2 were placed in a 1.0
At this temperature, calculate the number of moles of NO2(g) that must be added to 2.76 mol of SO2(g) in order to form 1.20 mol of SO3(g) at equilibrium.
What is the potassium ion concentration in a 2.5 m k2so4 aqueous solution
Which one of the following pairs of gases contains the same number of molecules (a) 16 g of O2 and 14 g of N2 (b) 8 g of O2 and 22 g of CO2 (c) 28 g of N2 and 22 g of CO2 (d) 32 g of O2 and 32 g of
For a cyclic process, q/t=delta s, calculate delta s when 2 mol of water vapor at 200C at 1atm undergoes a reversible cyclic process for which q=-145 j/mol
This was a question on my Mastering Chemistry homework. It's from Tro's Cha: Determine the pH of the following two-component solution: 0.260 M NH4NO3 and 0.102 M HCN
What volume and mass of the ethanol/water mixture did you collect from the simple distillation
1.00 mol of glucose was dissolved in water to form 1.00 L of solution at 298 K and 1 bar. Calculate free energy of mixture. Data for water: density 1.00 g/cm3, molar mass 18.02 g/mol, ?fGo(H2O,l) =
What is the pH of a 0.17 M solution of oxalic acid, H2C2O4. The Ka1,2 values of oxalic acid are 5.6 x 10-2 and 5.4 x 10-5.
How many grams of sodium formate, NaCHO2, would have to be dissolved in 1.1 L of 0.20 M formic acid (pKa 3.74) to make the solution a buffer for pH 3.82
Calculate the amount of water (in grams) that must be added to each of the following substances to produce the indicated solution 8.10g of urea(NH2)2CO in the preparation of 21.8 percent by mass sol
Find the number of moles of water that can be formed if you have 158 mol of hydrogen gas and 74 mol of oxygen gas. Express your answer with the appropriate units.
The initial disappearance of silver nitrate in water indicates a chemical reaction occurred The color change of the solution indicates a chemical reaction occurred A chemical reaction occurred when
The energy diagram shown represents the chemical reaction between solid ammonium chloride and solid barium hydroxide octahydrate: 2NH4Cl(s)+Ba(OH)2 * 8H2O(s)-----2NH3(aq)+BaCl2(aq)+10H2O(l)
What is the Gibbs free energy for this reaction at 5546 ? Assume that and do not change with temperature. At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium