1) given the following equation : Na2O 2Hl__>2Nal H2O (501.6KJ)
a) 1f 9g of Nal are formed by the process, how much heat(q)will be involved?
b) state whether the reaction is endorthermicor exothermic
To determine the amount of heat involved in a reaction and whether it is endothermic or exothermic, you need to understand the concept of enthalpy (heat) changes in chemical reactions.
The equation you provided represents a chemical reaction:
Na2O + 2Hl -> 2Nal + H2O (ΔH = -501.6 kJ)
a) To calculate the amount of heat (q) involved when 1 mol of Nal is formed, we will use the given enthalpy change (-501.6 kJ).
Step 1: Determine the molar ratio between Nal and the overall reaction.
From the balanced equation, we see that 2 mol of Nal are formed for every 1 mol of Na2O reacted. Therefore, the mole ratio is 2:1, Nal to Na2O.
Step 2: Convert the given moles of Nal (1f / 9g) into moles of Na2O.
To convert grams to moles, we need to know the molar mass of Nal. The molar mass of Nal (sodium iodide) is about 149.89 g/mol.
Given: 1f = 9g
Using the molar mass conversion:
(9g) * (1 mol / 149.89 g) ≈ 0.060 mol Nal
Step 3: Calculate the heat (q) involved using the stoichiometry and the given ΔH.
The molar ratio tells us that for every 2 moles of Nal formed, there is -501.6 kJ of heat released.
So, for 0.060 mol of Nal formed, the amount of heat released (q) can be calculated using the ratio:
(0.060 mol Nal) * (-501.6 kJ / 2 mol Nal) ≈ -15.048 kJ
Therefore, approximately -15.048 kJ of heat will be involved when 9 grams of Nal are formed.
b) To determine whether the reaction is endothermic or exothermic, we need to examine the sign of the ΔH value.
In this case, the ΔH value is -501.6 kJ (negative sign indicates exothermic).
Since the ΔH is negative, the reaction is exothermic.
You have an arrow but no + signs.
501.6 kJ x 9/2*molar mass NaI = heat (in kJ) involved.
You need to clarify the 501.6 kJ before I can tell you if it is exothermic or endothermic.