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Determine the empirical formula of a hydrocarbon which has 92.24% C and 7.76% H. If 0.500 g of this hydrocarbon occupies 0.086 L at STP, determine the molecular weight of the compound.
A saline solution contains 171 mEq/L each of Na+ and Cl-. how many moles of each of Na+ and Cl- are in 1.50 L of the saline solution.
Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ? CO(g) + H2O(g) The equilibrium concentrations of the reacting species.
What volume of a concentrated HCl solution, which is 36.0% by mass and has a density of 1.179 g/cm3, should be used to make 5.1 L of an solution with a pH of 1.5.
The Cl^- concentration in the water analysis given has been questioned. What concentration of Cl^- (mg/L) would make the cations and anions balance?
The tabulated mass of Cl is 35.45 amu. The two dominant isotopes of naturally occurring Cl are 35Cl (34.97 amu) and 37Cl (36.97 amu).
A 2.32 L balloon contains helium at 1.00 atm and 25°C. How many grams of helium are contained in the balloon.
Compute the number of gms of CoCl2 that would be needed to prepare the solutions:(a) 550 mL of a 1.75 M solution (b) 210 mL of a 0.0180 M solution.
Determine how many milligrams of H 2 O are present in sample If the freezing point of a 100.0g sample of 2-methyl-2-propanol =24.59C?
A swimming pool contains 88,000 liters of water and it having a surface area of 5 meters by 10 meters. It is observed that when this swimming pool is heated by the Sun for six hours.
How many moles of O2 are needed to consume 0.52 mol of Mg in the following unbalanced reaction? Mg + O2-> MgO
Compute the activation energy for the flashing process. When At 29 o C the average rate is 3.3 flashes every 10 seconds; at 23 degree Celsius the average rate
Considering given equation as P4(s) + 5 O2(g) P4O10(s) where ΔH = -3013 kJ/mol you just need to compute the heat evolved when 436 grams of white Phosphorous (P4)burns in air according to the given equation as above.
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