Question 1 You add 10.0 mls of 0.100 M H2SO4(aq) to 10.0 mls of 0.100 M NaOH(aq)

Question

Question 1 You add 10.0 mls of 0.100 M H2SO4(aq) to 10.0 mls of 0.100 M NaOH(aq). The products are: Select one: a. Na2S(s) and H2O(l) b. H2S(g) and Na2SO4(aq) c. Na2SO4(aq) and H2O(l) d. H2O(l) and NaSO4(aq) Question 2 Using the information from question 1, what are the stoichiometric coefficients for the reactant and products if you leave water as the last product? Select one: a. 1, 2, 1, 2 b. 2, 1, 2, 1 c. 1, 1, 1, 1 d. 1, 2, 1, 1 Question 3 You add 10.0 mls of 0.100 M H2SO4(aq) to 10.0 mls of 0.100 M NaOH(aq). How many moles of water are formed? Hint: Is there a limiting reagent? Select one: a. 0.00200 moles b. 0.00100 moles c. 0.200 moles d. 0.100 moles

Explanation / Answer

a. moles are conserved (moles of reactants are equal to moles of products). False. Think of decomposition reactions H2CO3 --------> CO2 + H2O If 1 mole H2CO3 decomposes you get 1 mole CO2 and 1 mole H2O 1 mole reagent ------> 2 moles product c. the stoichiometric coefficients of reactants equal the stoichiometric coefficients of products. False, Since the stoichiometric coefficients represent how many moles of each reagent and product are consumed/produced then this statement is basically a) re-worded. N2 + 3H2 ------> 2NH3 1 mole N2 + 3 moles H2 ----------->2 mole NH3 4 moles reactants ----------------------> 2 moles products d. the concentration(s) of reactants equal the concentration(s) of products. False, If the number of moles can be different on each side of the arrow then so can the concentration. Question 3 You add 10.0 mls of 0.100 M H2SO4(aq) to 10.0 mls of 0.100 M NaOH(aq). How many moles of water are formed c

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