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An impure sample of copper sulfate weighing 5.52 grams was dissolved in water and allowed to react with excess zinc. CuSO4(aq) + Zn(s) = ZnSO4 (aq) + Cu(s) What is the percent CuSO4 in the sample if 1.49 grams of metallic copper was produced?
a. 42.1%
b. 48.3 %
c. 55.5 %
d. 67.6 %
e. 73.5 %
Calculate the density of N2 at STP, (a) using the ideal-gas law and (b) using the molar volume and molar mass of N2.
Write an equation for this reaction? which species acts as the nucleophile? Which species acts as the electrophile?
Moles of carbonate in limestone? 2. % CaCo3 in limestone (Equation 2)?
What is the enthalpy of reaction, (triangle) H, for the formation of Tungsten carbide, WC, from the elements? W(s) + C(graphite) -> WC(s)
What mass of Cu and of N (in grams) are contained in 250.7 g of sample that is 75.4% pure Cu(NO3)2 by mass. (Assume that the impurities do not contain Cu and N.)
What is the pE value in an acid mine water sample having [Fe3+] = 6.79E-3 M and [Fe2+] = 4.14E-4 M?
if 24g mg is used and the percentage yield is 95 how many grams of magnesium hydroxide should be
Complete and balance the equation for this reaction in acidic solution. Phases are optional.
Given the following balanced reaction, if a mixture of 1.50 mol of Al and 3.00 mol of Cl2 are allowed to react, how many moles of AlCl3 are formed, assuming a 75% yield
Calculate the value of heat of vaporization for this liquid Calculate the normal boiling point of this liquid.
HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient water to yield 1.00 L of solution
What is the total mass of each of these elements in the Earth's crust (1 t = 1000kg)?
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