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Solve the following problem. Your solution should follow the ICE strategy and your final answer should have the correct units and number of significant figures.
For the reaction H2 + I2 -><- 2 HI at equilibrium, the 5 L reaction vessel contains 2.0 mol of H2, 4 mol of I2, and 3 mol of HI. How many moles of H2 need to be added to increase the concentration of HI to 0.84 mol/L?The biggest problem I'm running into is how to complete the ICE chart for the columns Change and Revised Equilibrium. I don't know where those numbers come from.
A particular system is doing work on the surroundings as well as gaining heat from the surroundings. What can be said about the values of q (heat) and w (work) for this system?
If 5 moles of propane and 10 moles of oxygen are sealed in a container and burned, which reactant will be the limiting reactant, and how many moles of carbon dioxide will be produced?
The highest possible oxidation state for halogens is +7 and the lowest possible is -1. Which of the following could not disproportionate?
Determine the final concentration if a 144-mL portion of that solution is diluted using water of 143 mL ?
Compute mass of Carbon dioxide formed from the decomposition of 59.0 grams of NaHCO 3 ?
A solution of ethanol (C2H5OH) in water is prepared by dissolving 63.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 255.0 mL of solution. What is the molarity of the ethanol in this solution?
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
What is the osmotic pressure of a solution made from dissolving 85.0g of glucose in 800ml of water at 19.0 C.
If 20.8 mL of NO2 gas is completely converted to N2O4 gas under the same conditions, what volume will the N2O4 occupy?
Calculate ΔH° for the reaction -> 2 K(s) + 2 H2O(l) 2 KOH(aq) + H2(g) A 4.85-g chunk of potassium is dropped into 1.06 kg water at 24.0°C.
In solving weak acid equilibrium problems to find [H+] or pH, a major assumption is usually made. This major assumption can be represented by the following
Calculate the number of grams of sulfuric acid present in the mixture after the reaction is complete.
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