Answer:Is sugar water a mixture or a compound? Define mixtures and compounds, and explain how without tasting it, Nicole can test to make sure she is using the sugar water in the glaze. The sugar-water is a mixture because it is chemically bonded, not chemically combined. A mixture is something that has 2 substances or more. hope this helps
Explanation:
Answer:
a) Equilibrium will shift to the left i.e. reactants
b) K will increase with increase in temperature
Explanation:
The given reaction is:
C6H12O6 + 6 O2 ↔ 6 CO2 + 6 H2O ΔH = -2816 kJ/mol
a) As per Le Chatelier's principle, for a reaction at equilibrium any changes in temperature, pressure or concentration will shift the equilibrium in a direction so as to undo the effect of the induced change.
The given reaction is exothermic (since ΔH is negative) i.e. it accompanied by the release of heat and hence an increase in temperature. Therefore, if the temperature is increased the equilibrium will shift in the opposite direction i.e. towards the left or towards the reactants.
b) The equilibrium constant (K) and temperature T are related via the Van't Hoff equation:
![[ln\frac{K2}{K1}=\frac{-\Delta H}{R}[\frac{1}{T2}-\frac{1}{T1}]](https://tex.z-dn.net/?f=%5Bln%5Cfrac%7BK2%7D%7BK1%7D%3D%5Cfrac%7B-%5CDelta%20H%7D%7BR%7D%5B%5Cfrac%7B1%7D%7BT2%7D-%5Cfrac%7B1%7D%7BT1%7D%5D)
In the given reaction, ΔH is negative and the condition is T2>T1
Therefore, K2 > K1
The value of equilibrium constant will increase with increase in temperature
i dont know how to remove my answer so ignore this
Answer:
There is 52.33 grams of water produced.
Explanation:
Step 1: Data given
Mass of propane burned = 32.00 grams
Molar mass of propane = 44.1 g/mol
Oxygen is in excess
Molar mass of water = 18.02 g/mol
Step 2: The balanced equation
C3H8 + 5O2 → 4H2O + 3CO2
Step 3: Calculate moles of propane
Moles of propane = mass propane / molar mass of propane
Moles of propane = 32.00 grams / 44.1 g/mol
Moles of propane = 0.726 moles
Step 4: Calculate moles of H2O
Propane is the limiting reactant.
For 1 mol of propane consumed, we need 5 moles of O2 to produce 4 moles of H2O and 3 moles of CO2
For 0.726 moles of propane we'll have 4*0.726 = 2.904 moles of H2O
Step 5: Calculate mass of H2O
Mass of H2O = moles of H2O * molar mass of H2O
Mass of H2O = 2.904 moles * 18.02 g/mol
Mass of H2O = 52.33 grams
There is 52.33 grams of water produced.
