Hydrogen sulphide, H₂S reacts with excess oxygen to produce sulphur dioxide. SO₂ and water. (b) (c) Write the balanced equation for the above reaction. Calculate the number of moles of H₂S required to form 4.22 mol of SO₂ Calculate the volume of oxygen consumed if 1.00 mol of H₂S was reacted at STP.

Hydrogen sulphide, H₂S reacts with excess oxygen to produce sulphur dioxide. SO₂ and water. (b) (c) Write the balanced equation for the above reaction. Calculate the number of moles of H₂S required to form 4.22 mol of SO₂ Calculate the volume of oxygen consumed if 1.00 mol of H₂S was reacted at STP.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What volume (in mL, at 373 K and 5.34 atm) of oxygen gas is required to react with 6.69 g of Al?
How many grams of sodium hydrogen carbonate decompose to give 28.7 mLmL of carbon dioxide gas at STP? 2NaHCO3(s)⟶ΔNa2CO3(s)+H2O(l)+CO2(g)
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?
According to the balanced equation, how many grams of aluminum are necessary to produce 1.50 Liters of hydrogen gas at STP? 2 Al(s) + 6 HCl(aq) --> 2 AlCl3(aq) + 3 H2(g)
According to the following chemical equation, how many liters at STP of hydrogen gas are needed to make 3.00 tons of iron? (2000 lbs. = 1 ton; 454 g = 1 lb.) [Hint: The equation is not balanced.] %D Fe,O3 + Н2 Fe + Н.О omic
A flask of volume 0.753 L contains a sample of chlorine gas, Cl2, with a pressure of 198 Torr at 25.8 degrees C What mass of sodium, in grams, is required to completely react with the chlorine to make sodium chloride? 2 Na (s) + Cl (g) - - > 2 Na C1 (s)
6. A quantity of solid sodium peroxide is reacted with excess water. The products of the reaction are aqueous sodium hydroxide and oxygen gas. (a) If 65.0 mL of oxygen gas at STP and 150.0 mL of sodium hydroxide solution resulted from the reaction, what is the molarity of the sodium hydroxide? (b) How many grams of sodium peroxide were used in problem 6(a)? (c) What would be the answer to question 6(a) if 84.5 mL of oxygen gas was collected at 35°C and 745 torr?
Given 25.4L of S2(g) at STP, how many moles are present?
What volume of O2 (MW = 32.00 g/mol) at STP is required for the complete combustion of 152.26 g CS2 (76.13 g/mol)?
The concentration of an old solution of hydrogen peroxide is being tested because hydrogen peroxide decomposes over time. The following reaction is catalyzed by potassium iodide and used to determine the concentration. If 3.0 ml of the peroxide solution is tested and produces 55 ml of O2(g) at 750 mm Hg and 23˚C, how many grams of hydrogen peroxide were in the solution? 2 H2O2(aq) à 2 H2O(l) + O2(g)
When 25.0 g of Zn reacts, how many L of H2 gas is formed at 25 °C and a pressure of 854 mmHg?
How many grams of sodium hydrogen carbonate decompose to give 27.6 mLmL of carbon dioxide gas at STP? 2NaHCO3(s)⟶ΔNa2CO3(s)+H2O(l)+CO2(g)