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A 0.456 gram sample of an unknown monoprotic acid (let's call it HZ) was dissolved in some water . Then the acidic solution was titrated to the equivalence point with 32.5 mL of 0.174 M KOH. What is the molecular weight of the unknown acid HZ?
The system CO2(g) + H2(g) *) H2O(g) + CO(g) is at equilibrium at some temperature. At equilibrium a 4.00 L vessel contains 1.00 mole CO2, 1.00 mole H2, 2.40 moles H2O, and 2.40 moles CO.
Calculate the volume of a balloon at the final temperature if this balloon at temperature of 279K and an initial volume of 2.3L is warmed to 406K.
2 g of a hydrocarbon fuel is burned in a colrimeter that contains 250 grams of water initially at 25 degrees celcius. After the combustion, the temperature is 26.55 degrees celcius.
A mixture of 0.1079 M CO (g) and 0.1079 M H2O(g) was allowed to react and come to equilibrium at some temperature. If Kc = 5.668, what is the equilibrium molar concentration of H2 for the reaction.
Calculate the values of E for the cell when the following volumes of the Ce^4+ titrant have been added. (Activity coefficients may be ignored as they tend to cancel when calculating concentrations of ratios.
Dissolves via the reaction and the temperature of the solution raises to twenty six degree celsius.compute the enthalpy change, , for this reaction per mole.
Calculate the Root Mean Square Speed and its average kinetic energy per molecule of Nitrogen and water vapor
Calcium carbide reacts with water to form acetylene and calcium hydroxide. From the following enthalpy data calculate Delta Hf for CaC2
Suppose that an excess of propane, C3H8 burns in 320 g of O2. How many moles of H2O will be formed? C3H8 + 5 O2 → 3 CO2 + 4 H2O
What mass of calcium metal could be obtained from one kg of limestone that is 50.0% pure CaCO3?
The enthalpy change for converting 1.00 mol of ice at -50.0 degrees C to water at 70.0 degrees C is ____ Kj. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-k and 1.84 J/g-k, respectively.
Assume that a reaction takes place at 296 K and 306 K. What must the activation energy be for the rate constant to double as described.
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