How many grams of Ag20 are required to produce 5.65 L oxygen gas via decomposition at 102.3 kPa and 175 ° C² ? 2Ag₂O 4Ag +O2

How many liters of sulfur dioxide gas can be produced at STP by the addition of 9.62 mol of hydrochloric acid (HCl) to sodium sulfite if sodium chloride and water are also produced?

A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based L-atm on experimentally collected data, the student calculates R to equal 0.0832 mol·K L-atm Ideal gas law constant from literature: 0.08206 mol·K (a) Determine the percent error for the student's R-value. Percent error = % (b) For the statements below, identify the possible source(s) of error for this student's trial. The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but does not dislodge it. The student does not clean the zinc metal with sand paper. The student does not equilibrate the water levels within the eudiometer and the beaker at the end of the reaction. The water level in the eudiometer is 1-inch above the water level in the beaker. The student uses the barometric pressure for the lab to calculate R.

Predict the volume of oxygen (at 25 degrees Celsius and 743 mm Hg) that will be liberated if 1.00g of sodium peroxide reacts with excess water via the following: 2Na2O2 (s) + 2 H2O (l)--> O2 (g) + 4 NaOH (aq)

Freon-12 (CF2Cl2), widely used as a refrigerant and aerosol propellant, is a dangerous airpollutant. In the troposphere, it traps heat 25 times as effectively as CO2, and in thestratosphere, it participates in the breakdown of ozone. Freon-12 is prepared industrially byreaction of gaseous carbon tetrachloride with hydrogen fluoride. Hydrogen chloride gasalso forms. How many grams of carbon tetrachloride are required for the production of16.0 dm3 of Freon-12 at 27°C and 1.20 atm?

lithium reacts with H2O to produce hydrogen.(a) Write a balanced chemical equation for the reaction, using the smallest integer coefficients possible. Write states in brackets. (Hint: LiOH is the second product.) (b) Calculate the mass of pure Li that will furnish 16.3 L of hydrogen at a pressure of 0.860 atm and a temperature of 30.4°C.