A reaction between liquid reactants takes place at -16C in a sealed, evacuated vessel with a measured volume of 45L. Measurements show that the reaction produced 34g of sulfur hexafluoride gas. Calculate the pressure of sulfur hexafluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Be sure your answer has the correct number of significant digits.

0.11 atm

Explanation:

Given data

First, we will calculate the moles (n) of sulfur hexafluoride, considering its molar mass is 146.06 g/mol.

34 g × (1 mol/146.06 g) = 0.23 mol

Then, we can calculate the pressure (P) of sulfur hexafluoride using the ideal gas equation.

P × V = n × R × T

P = n × R × T / V

P = 0.23 mol × (0.082 atm.L/mol.K) × 257 K / 45 L

P = 0.11 atm

if you mean hydrogen and oxygen then water is the product

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.