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Problem- An equilibrium mixture contains 0.600 mol of each of the products (carbon dioxide and hydrogen gas) and 0.200 mol of each of the reactants (carbon monoxide and water vapor) in a 1.00-L container How many moles of carbon dioxide would have to be added at constant temperature and volume to increase the amount of carbon monoxide to 0.300 mol?
CO(g) + H2O(g) <---> CO2(g) + H2(g)
As much detail as feasible is really appreciated
Splitting patterns and integrations may be used more than once, or not at all, as needed. Likewise, some bins might remain blank. Note that peak heights are arbitrary and do not indicate proton integrations.
a v 535 ml at 1.00 atm. what is the volume at 675 torr?b v 2.07 l at 110.9 kpa. what is the volume at 0.992 atm?c v
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The overall reaction for the corrosion of iron by oxygen is given by the following reaction. 4Fe (s) + 3O2 (g) ?? 2Fe2O3 (s) Compound ?H° (kJ/mol) S° (J/mol K) Fe (s) 0 27 O2 (g) 0 205 Fe2O3 (s) -826 90 Calculate the equilibrium constant, Keq, for..
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Problem- A 4.82g sample of iron is heated to 84.3 degrees Celsius. A 1.25g sample of gold is heated to 95.1 degrees Celsius. Both of these metals are added to 9.47g of cold water that is initially at 14.5 degrees Celsius.
An apparatus to be used in a decomposition study was filled with N2 gas at 400.00 mm Hg and 400.0 deg C. The volume of the apparatus was 400.0 mL.
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In an endothermic reaction, in going from the reactants to the products at the same temperature, the value of q is negative.
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