3. Ca(OH)2 (aq) + H2SO4 (aq) + 2 H₂O (1) + CaSO4 (aq) (This is LIMITING REACTANT: H2SO4 is the Limiting Reactant) Reaction Type: Neutralization Grams of Product (List the Product and the Amount): 0.180 g H₂O and 0.681 g CaSO4 ? g H₂O 1.839 g Ca(OH)2 x ? g H₂O 25.0 mL H₂SO4 x 1 mol Ca(OH)2 X 74.10 g Ca(OH)2 2 mol H₂O 1 mol Ca(OH)2 x 18.02 g H₂O = 0.8944 g H₂O 1 mol H₂O 1 L H₂SO4 x 0.200 mol H₂SO4 x 2 mol H₂O x 1000 mL H₂SO4 1 L H2SO4 1 mol H₂SO4 18.02 g H₂O = 0.180 g H₂O 1 mol H₂O ONLY USE THE Limiting Reactant TO DETERMINE THE AMOUNT OF THE REMAINING PRODUCT(S). ? g H₂O 25.0 mL H₂SO4 x 1 L H₂SO4 x 0.200 mol H₂SO4 x 1 mol CaSO4 x 136.14 g CaSO4 = 0.681 g CaSO4 1000 mL H₂SO4 1 L H₂SO4 1 mol H₂SO4 1 mol CaSO4 YOU MUST CALCULATE THE AMOUNT OF EXCESS REACTANT LEFT OVER AT THE END OF THE REACTION!!!!!!!

According to the following reaction, how many moles of nitrogen monoxide will be formed upon the complete reaction of 26.6 grams of nitrogen gas with excess oxygen gas ? nitrogen(g) + oxygen(g) => nitrogen monoxide(g) 57.0 grams O 1.90 moles 0475 moles 0.950 moles hp

Which term describes the study of the mass and mole relationships between reactants and products in a chemical reaction? theoretical yield percentage yield stoichiometry O actual yield

Nitrogen (N,) gas and hydrogen (H,) gas react to form ammonia (NH,) gas. Suppose you have 9.0 mol of N, and 5.0 mol of H, in a reactor. Suppose as much as possible of the N, reacts. How much will be left? Round your answer to the nearest 0.1 mol. O mol Continue

Which of the following is NOT true about "yield"? * The percent yield is the ratio of the actual yield to the theoretical yield. The value of the actual yield must be given in order for the percent yield to be calculated. The actual yield may be different from the theoretical yield because insufficient limiting reagent was used. The actual yield may be different from the theoretical yield because reactions do not always go to completion.

What is an indicator? What is a buffer?

For the reaction of nitrogen dioxide with water to form nitric acid and nitrogen monoxide, what is the sum of the coefficients of the balanced equation?

match the folowing terms. one answer will not be used. Left Side: limiting reactant actual yield theoretical yield percent yield mole ratio Right Side (match) maximum amount of product that could produced relationship between two different components of a balanced equation the reaction component that is consumed entirely the reaction component that is present in excess the actual yield divided by the theoretical yield 100 times amount of product physically produced from a reaction

[References] Use the References to access important values if needed for this question. For the following reaction, 0.169 moles of chlorine gas are mixed with 0.277 moles of sodium iodide. chlorine(g) + sodium iodide(s) sodium chloride(s) + iodine(s) What is the formula for the limiting reagent? What is the maximum amount of sodium chloride that can be produced? moles Submit Answer Retry Entire Group 6 more group attempts remaining

In the balanced equation for the complete neutralization of phosphoric acid by calcium hydroxide, the mole:mole ratio of phosphoric acid to calcium hydroxide is