In the laboratory, hydrogen gas is usually made by the following reaction: Zn(s) + 2 HCl(aq) → H2(g) + ZnCl2(aq) How many liters of H2 gas, collected over water at an atmospheric pressure of 752 mm Hg and a temperature of 21.0°C, can be made from 2.566 g of Zn and excess HCl? The partial pressure of water vapor is 18.65 mm Hg at 21.0°C. a) 0.959 L b) 0.0701 L c) 0.981 L d) 0.939 L

Determine the mass of oxygen in a 6.8-g sample of Al2(SO4)3. Express your answer to two significant figures and include the appropriate units.

a 2.802g sample of an unknown pure metal (M) is added to a 0.2 L solution of 2 mol/L H2SO4(aq). The metal reacts with the acid until the metal is completely gone to form M3+(aq) ion in the solution and produces hydrogen gas that is collected. The hydrogen gas that is collected over water that is isolated from the reaction has a volume of 0.82 L at 25 degrees Celsius and a total pressure of 704.0 mmHg. How many moles of H2(g) are produced? Write a balanced equation for the reaction of M with H2SO4(aq). What is the identity of metal M?

When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction CaCO3(s)→CaO(s)+CO2(g)CaCO3(s)→CaO(s)+CO2(g) What is the mass of calcium carbonate needed to produce 65.0 LL of carbon dioxide at STP?

How many moles of carbon dioxide, CO2, are produced if the reaction conditions are 325 K, 1.6 atm, and 5.3 L? If the carbon dioxide, CO2, is produced according to the chemical reaction shown below, how many grams of propane, C3H8, were required?   2 C3H8(g) + 5 O2(g) → 3 CO2(g)  + 4 H2O(g)   For the calculations in this module, the molar mass of an element will be rounded to the hundredths place (0.01 g).

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

Consider the following balanced reaction: Mg(s) + 2HCI(g) → MgCl2(aq) + H2(8) Calculate the volume of H2 produced when 48.62 grams of magnesium react with the excess of hydrochloric acid at 20°C and 741mm Hg. O 22.4 L O 24.7 L O 44.8 L O 49.3 L O 94.5 L

Ammonia Production Ammonia is often formed by reacting nitrogen and hydrogen gases. How many liters of ammonia gas can be formed from 13.7 L of hydrogen gas at 93.0°C and a pressure of 40.0 kPa?

please answer the question and show your work 5a. An automobile airbag inflates when sodium azide (NaN3) is converted to sodium (Na) and N2 gas according to the BALANCED equation, 2 NaN3 → 2 Na + 3 N2.  What volume in liters (L) of N2 gas will be produced if 115 g of NaN3 completely reacted at STP (standard temperature and pressure).   Molar mass of NaN3 = 65.02 g/mol        1 mol of any gas at STP = 22.4 L

How many grams of NaClO3 were decomposed?