<u>Answer:</u> The amount of hydrogen sulfide needed is 6.2 moles and amount of sulfur dioxide gas produced is 6.2 moles
<u>Explanation:</u>
We are given:
Moles of oxygen gas = 9.3 moles
The chemical equation for the reaction of oxygen gas and hydrogen sulfide follows:
<u>For hydrogen sulfide:</u>
By Stoichiometry of the reaction:
3 moles of oxygen gas reacts with 2 moles of hydrogen sulfide
So, 9.3 moles of oxygen gas will react with = of hydrogen sulfide
<u>For sulfur dioxide:</u>
By Stoichiometry of the reaction:
3 moles of oxygen gas produces 2 moles of sulfur dioxide
So, 9.3 moles of oxygen gas will produce = of sulfur dioxide
Hence, the amount of hydrogen sulfide needed is 6.2 moles and amount of sulfur dioxide gas produced is 6.2 moles
Because as the air hits the charcoal it becomes ash and changes color.
Answer:
445.8 J of heat is absorbed by the water
Explanation:
Step 1: Data given
Mass of water = 32.0 grams
Initial temperature = 19.50 °C
Final temperature = 22.83 °C
Specific heat of water = 4.184 J.g°C
Step 2: Calculate the amount of heat absorbed by the water
Q = m*c*ΔT
⇒with Q = the heat absorbed = TO BE DETERMINED
⇒with m= the mass of water = 32.0 grams
⇒with c= the specific heat of water = 4.184 J/g°C
⇒with ΔT = the change of temperature = T2 - T1 = 22.83 °C - 19.50 °C = 3.33 °C
Q = 32.0 * 4.184 * 3.33
Q = 445.8 J
445.8 J of heat is absorbed by the water