How many grams of fluorine are needed to react with 8.5g of phosphorus?

Step 1: write the equation:

                                          P₄(s) + 6F₂(g) → 4PF₃(g) 

Step 2: Molar mass of P₄ = 30.97 g/mol × 4 = 123.88 g/mol

Step 3: Number of moles of phosphorus

                                                    n = m/M 

                                                    n = 8.5 g/123.88g/mol

                                                    n = 0.07 moles

Step 4: 0.07 × 12 = 0.84 moles of fluorine.

Fluorine is diatomic gas so we multiplied the number of moles by 12.

Step 5: To find the mass of fluorine we multiply the number of moles with the molar mass.

                            Mass of fluorine = 0.84 ×  228 

                                                        = 191.52 grams.

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.