I already have the first two answers I'm just stuck with the last two. A student demonstrates the reaction by mixing 25.00 g of H2SO4 with 25.00 g of CaCO3. a. How many moles of each reactant does the student mix? 2.55 x 10^-1 mol H2SO4 Approx. 2.5 x 10^-1 mol CaCO3 b. Identify the limiting reactant. Explain how you know this. CaCO3 c. Calculate the theoretical mass of the excess reactant. d. Soon after mixing the reactants, the student determines that 33.17 g of CaSO4 was produced by the reaction. Is this a reasonable result? Show calculations to defend your answer.

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl+4h2o enter the elemental symbol. view available hint(s) is reduced

Chemical energy is a form of a. kinetic energy only. b. both potential and kinetic energy. c. neither potential nor kinetic energy. d. potential energy only. reset

How can one make a supersaturated solution? (apex)