For each of the following balanced chemical equations, calculate how many moles of each product would be produced by the complete conversion of 0.25 mol of the reactant indicated in boldface. State clearly the mole ratio
used for the conversion.
a. 3PbO(s) + 2Al(s) 3Pb(s) + Al203(s)
b. C2H2(g) + 2H2(g) C2H6(g)
c. BaO2(s) + 2Na(s) Na2O2(s) + Ba(s)
d. 2CH4(g) + 302(g) 2CO(g) + 4H2O(l)

According to each substances heat of fusion, which of the items below requires more heat to be added per gram of substance to go from solid to liquid? silver sulfur water lead

For a research project, a student decided to test the effect of the lead(ii) ion (pb2+) on the ability of salmon eggs to hatch. this ion was obtainable from the water‐soluble salt, lead(ii) nitrate, which the student decided to make by the following reaction. pbo(s) + 2 hno3(aq) → pb(no3)2(aq) + h2o losses of product for various reasons were expected, and a yield of 86.0% was expected. in order to have 5.00 g of product at this yield, how many grams of pbo should be reacted? (assume that sufficient nitric acid, hno3, would be used.)

1.17 mol hcl and 2.5 mol naoh react according to the equation hcl + naoh -> nacl + h2o . if the limiting reactant is hcl, determine the amount of excess reactant that remains. answer in units of mol.