Aqueous hydrobromic acid HBr will react with solid sodium hydroxide NaOH to produce aqueous sodium bromide NaBr and liquid water H2O.Suppose 61. g of hydrobromic acid is mixed with 44.1 g of sodium hydroxide. Calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

If excess chlorine gas reacts with a solution containing 20.0 grams of potasium bromide, how many liters of bromine gas can be produced?

A chemist needs to add 3.5 moles NaClNaClto a reaction. How much NaCl should she measure out in grams (g)? Round to two decimal places if necessary.      140.21g NaCl   204.54g NaCl   58.44g NaCl   0.60g NaCl

Consider the following chemical reaction HCl (aq)  + HgNO3 (aq) à Hg2Cl2 (s) + HNO3 (aq) If 20.0 grams of HCl is mixed with 30.0 grams of HgNO3     Determine the excess reactant   The amount of the solid precipitate that was recovered equals to .................. grams , if the percentage yield from this reaction was determined to be 78.4%. Write the net ionic equation for the chemical reaction   Determine the type of this chemical reaction

Aqueous hydrobromic acid  HBr  reacts with solid sodium hydroxide  NaOH  to produce aqueous sodium bromide  NaBr  and liquid water  H2O . If  0.321g  of water is produced from the reaction of  3.2g  of hydrobromic acid and  2.1g  of sodium hydroxide, calculate the percent yield of water.Be sure your answer has the correct number of significant digits in it.

Consider the following unbalanced chemical reaction:  Br2 + F2 → BrF5 How many grams of fluorine gas (F2) would be required to completely react with 100.0 grams of bromine (Br2)?

A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. (0.19 L) 1 mL 10-³ 146.86 g mol 1.04 mL = ☐ x10 ロ･ロ X I 00

Let us explore a reaction with a limiting reactant. Here, zinc metal is added to a flask containing aqueous HCl, and H2 gas is a product.   The three flasks each contain 0.300 mol of HCl. Zinc is added to each flask in the following quantities: 4.90 g, 9.81 g, 19.6 g.  When the reactants are combined, the  inflates the balloon attached to the flask. The results are as follows: Flask 1: Balloon inflates completely, but some  remains when inflation ceases. Flask 2: Balloon inflates completely. No Zn remains. Flask 3: Balloon does not inflate completely. No Zn remains.   What mass of Zn was added to each flask? Mass = ? g (flask 1) Mass = ? g (flask 2) Mass = ? g (flask 3)

For the reaction Ca(s)+Cl2(g)→CaCl2(s) calculate how many grams of the product form when 21.4 gg of Ca completely reacts. Assume that there is more than enough of the other reactant.

[Tutorial: Limiting reactant stoichiometry] This question will walk you through the steps of calculating the mass of products produced based on your determination of the limiting reactant.   b) Step 2a: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 64.7 grams Al according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) c) Calculate the theoretical yield in grams Al₂O₃ from the complete reaction of 201 grams Fe₂O₃ according to the following balanced chemical equation: 2 Al(s) + Fe₂O₃(s) → Al₂O₃(s) + 2 Fe(s) d) Which of the following substances is the limiting reactant? e) What is the mass in grams of the excess Fe₂O₃ remaining after the partial reaction of 201 g Fe₂O₃ with 64.7 g Al? Give your answer to three significant figures.