When 56.8 g of lead reacts with 3.50 L of oxygen gas, measured at 1.00 atm...
16. How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts with 29.0 L of carbon dioxide gas, measured at 1.00 atm pressure and 25.0°C? (R-0.0821 L atm/(K mol)) CaO(s)+CO:(g) a. -3.11 x 102 kJ CaCO:(s); AHP = -178.3 kJ b. -1.74 x 10 kJ c. -5.22 x 102 kJ d. -2.11 x 10 kJ e. -5.17 x 103 kJ
15. In a mixture of helium and chlorine, occupying a volume of 12.8 L at 605,6 mmHg and 21.6°C, it is found that the partial pressure of chlorine is 143 mmHg. What is the total mass of the sample? a. 31.6 g b. 0.4 g c. 8.37 g d. 1.28 g e. 7.09 g 16. How much heat is liberated at constant pressure when 97.7 g of calcium oxide reacts with 29.0 L of carbon dioxide gas, measured at 1.00...
Consider the reaction. 2Pb(s)+O2(g)⟶2PbO(s) An excess of oxygen reacts with 451.4 g of lead, forming 386.1 g of lead(II) oxide. Calculate the percent yield of the reaction.
If a sample of oxygen gas, originally at 5.00 atm in 1.00 L, is heated in that container from 25.0°C to 175°C, what is the final pressure? A: 7.52 atm B: 0.714 atm C: 0.133 atm D: 35.0 atm
1. If nitrogen gas has a density of 1.14 g/L, and an unknown gas has a density of 4.2 g/L at the same temperature and pressure, what is the ratio of the rate of effusion of the known gas to the rate of effusion of nitrogen? 2. The combustion reaction for octane burning in oxygen is: 2 C8H18 (l) + 25 O2(g) → 16 CO2(g) +18 H2O(g) ∆H = -10869 kJ . Suppose an oxygen bomb calorimeter is loaded with oxygen...
When solid lead(II) sulfide reacts with oxygen gas, the products are solid lead(II) oxide and sulfur dioxide gas. A. Write the balanced equation for the reaction. Express your answer as a chemical equation. Identify all of the phases in your answer. B. How many grams of oxygen are required to react with 25.3 g of lead(II) sulfide? C. How many grams of sulfur dioxide can be produced when 56.8 g of lead(II) sulfide reacts? D. How many grams of lead(II)...
When 20.00 moles of H2(g) reacts with 10.00 mol of O2(g) to form 20.00 mol of H2O(1) at 25°C and a constant pressure of 1.00 atm. If 1366 kJ of heat are released during this reaction, and PAV is equal to -74.00 kJ, then AH° = +1366 kJ and AE = +1440 kJ. O AH° = +1366 kJ and AE° = +1292 kJ. O AH° = -1366 kJ and AE° = -1292 kJ. O AH° = -1366 kJ and AE°...
1 altm=101.32j A gas is confined to a cylinder under constant pressure of 3.50 atm. When the gas undergoes a particular chemical reaction, it releases 79 kJ of heat to its surroundings and expands from 22.0L to 75.2 L. Determine both AE and AH for this scenario.
An oxygen gas container has a volume of 20.0 L. How many grams of oxygen are in the container if the gas has a pressure of 887 mmHg at 24 ∘C? Mg metal reacts with HCl to produce hydrogen gas. Mg(s)+2HCl(aq)→MgCl2(aq)+H2(g) What volume of hydrogen at 0 ∘C and 1.00 atm (STP) is released when 9.40 g of Mg reacts? How many grams of magnesium are needed to prepare 6.90 L of H2 at 775 mmHg and 20 ∘C?
When sulfuric acid reacts with sodium bicarbonate, carbon dioxide gas is released. If 2.0 L of CO2 gas is collected at standard temperature and pressure, how many grams of sodium bicarbonate we consumed? (use ideal gas law - R = 0.0821 l*atm/mol*k) H2So4 (aq) + 2NaHCO3 (aq) -> Na2SO4 (aq) + 2H2O (I) + 2CO3 (g) a) 7.5 g b) 8.7 g c) 3.9 g d) 4.7 g