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A student performs the following gravimetric analysis of iron ions in a water system:Fe2+ (aq) + 2CO32- (aq) = FeCO3 (s)If this student used excess carbonate and obtained the following data, what was the original concentration in moles/L) of Fe2+ in the water sample? Total Volume of Solution: 100.00 mLMass of FeCO3 collected: 23.758 grams.Is this how you would solve it change 100 ml to .1 liters. 115.853x = 23.758 x .1 = .02 liters.
What volume of ammonia at 25 °C and 1.5 atm pressure is needed to produce 500 g of urea?
The molar stoichiometric ratio of nitrogen produced to ammonia reacted in the reaction equation is one to one, and the mol CO2/mol C6H12O6 = 2. How much (in g mol) (a) glycerol was produced and (b) how much biomass reacted to produce the 52.4 L of..
Question- Write the chemical equation that defines the normal boiling point of liquid phosphorous trichloride. What is the delta G degrees for the phase change at equilibrium? Estimate the normal boiling point of PCl3.
A mixture of 2.00 moles of H2, 3.00 moles of MH3, 4.00 moles of CO2, and 5.00 moles of N2 exert a total pressure of 350kPa. What is the partial pressure of each gas?
Problem- Compute change in H (delta H) and change in S for ice betweeen -10 degrees Celsius and +10 degrees Celsius knowing that
Problem- Derive the intergrates rate expression for a reaction which is 1/2 order in [A]. Derive an expression for t1/2
A sample of river water has a bicarbonate ion concentration of 1.0 × 10-4M. Calculate the total alkalinity for the sample in mmol/L.
Question- The Ksp of metal hydroxide Mg(OH)2 is 1.20 x 10-11. 1) What is the solubility of this compound in g/L
an aqueous ammonium chloride solution rather than sulfuric acidis used in the hydrolysis of the magnesium complex
How many grams of O2 gas would occupy a 400.0 liter container when the temperature is 300.0 K and the pressure is 2.20 atm?
What is w when a gas is compressed from 38.3 L to 28.8 L using a constant external pressure of 745 mmHg? (Remember to include a "+" or "-" sign as appropriate.)
Some of the best laboratory vacuum systems can pump down to as few as 9.0 multiplied by 109 molecules per cubic meter of gas. Calculate the corresponding pressure, in atmospheres, assuming a temperature of 25°C.
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