Answer:
1.368 grams of manganese dioxide must b added to HCl to obtain 385 mL of chlorine gas.
Explanation:
Using ideal gas equation:
PV = nRT
where,
P = Pressure of chlorine gas = 
1 atm = 760 Torr
V = Volume of chlorine gas = 385 mL = 0.385 L ( 1 mL - 0.001 L)
n = number of moles of chlorine gas = ?
R = Gas constant = 0.0821 L.atm/mol.K
T = Temperature of chlorine gas =25 °C= 25 + 273 K = 300 K
Putting values in above equation, we get:
According to reaction, 1 mole of chlorine gas is obtained from 1 mole of manganese dioxide ,then 0.01573 moles of chlorine gas will be obtained from :
of manganese dioxide
Mass of 0.01573 moles of manganese dioxide:
0.01573 mol × 86.94 g/mol = 1.368 g
1.368 grams of manganese dioxide must b added to HCl to obtain 385 mL of chlorine gas.
The answer would be 0.8 mol of x left over....
AND THATS IS WHY...refer to the pic below...
See if it is clear enough...
Answer:
D. Water and Carbondioxide
Explanation:
Combustion of organic compounds in the presence of excess Oxygen will liberate carbondioxide (CO2) and water vapour (H2O). This is an exothermic reaction because heat is liberated to the surroundings.
CnH2n+1OH(aq) + (3/2*n)O2(g) --> nCO2(g) + (n + 1)H2O(g)
Addition of Oxygen can also be termed as a redox reaction. In this case, alcohols are oxidised while the Oxygen is reduced.
Example, (propanol)
C3H7OH(aq) + 9/2O2(g) --> 3CO2(g) + 4H2O(g)
<span>If "hf" is the standard heat of formation, the Hf for Al is zero -- as it is for all elements in their standard state. The standard heat of formation for water is −285.8 kJ/mol. Thank you for posting your question here. I hope the answer helps. </span>
