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How many grams of solid magnesium nitrate should be added to 500 mL of 0.118 M of sodium nitrate in order to produce an aqueous 0.25 M solution of nitrate ions?
Write a balanced, net ionic equation for the reaction of Na2S(aq) and ZnSO4(aq) , also please include physical states and charges of ions.
Sulfur Dioxide reacts with oxygen to produce Sulfur trioxide in the presence of a catalyst. In an experiment carried out at 727 degrees Celsius
kp 1.78 at 250ordmc for the decomposition reaction pcl5g ? pcl3g cl2g. calculate the percentage of reactant that
CO +H2O ->
A chemical is placed in a beaker containing 20g of soil and 500 ml water. at equilibrium, the chemical is found in the soil at a concentration of 100mg/kg of soil. the equilibrium concentration of this same chemical in the water is 250µg/L.
The student adds 6 M NH3 to CuSO4 solution until the Cu 2+ ion is essentially all converted to Cu(NH3)4 2+ ion. The voltage of the cell goes up to 0.92 V and the Cu electrode is still negative. Find the residual concentration of Cu 2+ ion in the c..
given the balanced equation representing a reacction2c2h67o24co26h2odetermine the total number of moles of oxygen that
What is the equilibrium partial pressure of NO in the air at 1000K if the partial pressure of nitrogen is 0.80bar, the partial pressure of oxygen is 0.20bar and delta G for the following reaction is 77.772kj/mole
If atmospheric pressure suddenly changes from 1.00 atm to 0.898 atm at 298 K, how much oxygen will be released from 3.10 L of water in an unsealed container?
Integrate the expression b = 1/V (derivative of V / derivative of T) at constant pressure, assuming that b is independent of temperature. By doing so, obtain an expression for V as a function of T and b at constant P. b means beta
Question- At 25 °C only 0.0560 mol of the generic salt AB3 is soluble in 1.00 L of water. Define what is the Ksp of the salt at 25 °C
Assuming that the container is completely full, that the temperature is 20.7oC, and that the atmospheric pressure is 1.2atm, calculate the percent (by volume) of air that would be displaced if all of the liquid nitrogen evaporated
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