Zn (s) + H2SO4 (aq) --> H2 (g) + ZnSO4 (aq) You run a reaction and collect 166.3 mL of hydrogen gas from this reaction into a balloon. If the atmospheric pressure is 740.3 torr, and the temperature of the gas is 23.4°C, how many grams of Zn must have reacted.

Boron trifluoride gas is collected at 6.0 °C in an evacuated flask with a measured volume of 15.0 L. When all the gas has been collected, the pressure in the flask is measured to be 0.140 atm . Calculate the mass and number of moles of boron trifluoride gas that were collected. Be sure your answer has the correct number of significant digits. mass: g x10 mole: | mol ?

Zinc reacts with aqueous HCl to produce hydrogen gas (H2) according to the following reaction equation:Zn (s) + HCl (aq) → ZnCl2 (aq) + H2 (g)The hydrogen gas is collected over water. If you collected 260 mL of H2 at 25 oC, and the total pressure was 745 mm Hg, calculate the mass of H2 collected over water.

A 2.20 L container at 53.6 °C contains 6.21g N2⁢O3⁡(g). The N2⁢O3 gas decomposes completely, producing NO2⁢(g) and NO(g). Assuming the container volume and the temperature do not change, calculate the pressure of the gas mixture after the complete decomposition of N2O3.

Sometimes in lab we collect the gas formed by a chemical reaction over water (see sketch at right). This makes it easy to isolate and measure the amount of gas produced. 2 Suppose the CO₂ gas evolved by a certain chemical reaction taking place at 40.0 °C is collected over water, using an apparatus something like that in the sketch, and the final volume of gas in the collection tube is measured to be 51.0 mL. g x10 X 歐 Sketch of a gas-collection apparatus S collected gas Calculate the mass of CO₂ that is in the collection tube. Round your answer to 2 significant digits. You can make any normal and reasonable assumption about 2 the reaction conditions and the nature of the gases. water chemical reaction

A sample of gas contains 0.1700 mol of CH4(g) and 0.1700 mol of H2O(g) and occupies a volume of 19.2 L. The following reaction takes place:CH4(g) + H2O(g)3H2(g) + CO(g)Calculate the volume of the sample after the reaction takes place, assuming that the temperature and the pressure remain constant.

A helium-filled weather balloon has a volume of 506 L at 19.9°C and 758 mmHg. It is released and rises to an altitude of 5.40 km, where the pressure is 462 mmHg and the temperature is –14.1°C. The volume of the balloon at this altitude is ___ L.

In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition of sodium azide (NaN3) to its elements. A 69.9−g sample of sodium azide was decomposed, and the nitrogen gas generated was collected over water at 26°C. The total pressure was 748.5 mmHg. How many liters of dry N2 were generated?

The hydrogen gas evolved in a reaction between solid zinc and hydrochloric acid has been collected over water.  The volume of water displaced is equal to 0.587 L.  Given that the gas was collected at a temperature of 30.0°C and the atmospheric pressure was 738 torr, what mass (in mg) of hydrogen gas was collected?  (3 sf) =

A reaction between liquid reactants takes place at - 14.0 °C in a sealed, evacuated vessel with a measured volume of 40.0 L. Measurements show that the reaction produced 36. g of chlorine pentafluoride gas. Calculate the pressure of chlorine pentafluoride 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. pressure: |II atm