261.162 grams. Use the equation n=M÷Mr.
Answer:
There is 117.4 kJ of heat absorbed
Explanation:
<u>Step 1: </u>Data given
Number of moles CS2 = 1 mol
Temperature = 25° = 273 +25 = 298 Kelvin
Heat absorbed = 89.7 kJ
It takes 27.7 kJ to vaporize 1 mol of the liquid
<u>Step 2:</u> Calculate the heat that is absorbed
C(s) + 2S(s) → CS2(l) ΔH = 89.7 kJ (positive since heat is absorbed)
CS2(l) → CS2(g) ΔH = 27.7 kJ (positive since heat is absorbed)
We should balance the equations, before summing, but since they are already balanced, we don't have to change anything.
C(s) + 2S(s)---> CS2 (g)
ΔH = 89.7 + 27.7 = 117.4 kJ
There is 117.4 kJ of heat absorbed
Hello there!
From my calculations the answers are:
D. Mass
B. Gravity
B. Gravity
Hope This Helps You!
Good Luck :)
You need to specify the experiment to get an answer. However, most experiments require qualitative data (descriptive, non-numerical data) and quantitative data (measured, numerical data).
