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A compound contains 10.13% C and 89.87% Cl (by mass). Determine both the empirical formula and the molecular formula of the compound given that the molar mass is 237 g/mol.
Write the balanced net ionic equation for the reaction that occur in the following case. Ba(NO3)2 (aq) + K2SO4(q) Express your answer as a balanced net ionic equation.
Aluminum readily displaces hydrogen in sulfuric acid according the following balanced reaction: 2Al(s) + 3H2SO4(aq) = Al2(SO4)3(aq) + 3H2(g). How many moles of Al and how many moles
Centuries before any experiments had been carried out, philosophers had proposed the existence of the atom. Why are the proposals of these philosophers not considered theories?
Calcium concentrations in solutions may be determined by a complex-forming reaction with EDTA. The reaction takes place between Ca2+ and EDTA4- with a formation constant of 4.5 x1010.
how many moles of ammonia are produced? How many moles of H2 remain? How many Moles of N2 remain? What is the limiting reactant?
Make a list of the operations you will need to perform in order to display a spectrum of your food dye on the spectrophotometer.
Given the following equation, how many grams of PbCO3 will dissolve when 1.5L of 1.00 M H+ is added to 6.00g of PbCO3? PbCO3(s) + 2H+(aq) = Pb^2(aq)+ +H2O (l)+ CO2(g)
at 25.0degc a sample of xe gas occupies 531 ml in a piston-cylider apparatus when the external pressure is 337 torr. at
Calculate the change in entropy (in J/K) when a 44.0 g of nitrogen gas is heated at a constant pressure of 1.50 atm from 19.3 ºC to 86.5 ºC.
Given the data below for the reaction, 2 A + 2 B + 4 C => D + E + 3 F, Experiment Initial conc of A, mol/L Initial conc of B, mol/L Initial conc of C, mol/L Initial rate, mol/L.s 1 0.1 0.2 0.4 2 x 10-3 2 0.2 0.2 0.4 2 x 10-3 3 0.3 0.4 0.4 4 x 10-3..
1. assume that the specific heat of the waterh2o 1.00 cavg xc then calculate how many calories of heat are needed to
He decided to dry the alum by heating it strongly. Unfortunately he also drove off the waters of hydration. What is the mass of his remaining anhydrous salt?
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