Answer: The 234.74 grams of sample should be ordered.
Explanation:
Let the gram of 114 Ag to ordered be
The amount required for the beginning of experiment = 0.0575 g
Time requires to ship the sample = 4.2hour = 252 min(1 hr = 60 min)
Half life of the sample = = 21 min
The 234.74 grams of sample should be ordered.
The volume of carbon dioxide produced is : 5.4 L
<u>Given data:</u>
moles of propane = 0.080 moles
<h3>Determine the volume of Carbon dioxide produced </h3>
The chemical reaction
C₃H₈ + 5O₂ ---- > 3CO₂ + 4H₂O
From the reaction
I mole of C₃H₈ = 3CO₂
0.080 moles of C₃H₈ = 3 * 0.080 = 0.24
Applying the equation below to determine the volume of CO₂
Pv = nRT
= 0.24 * R * T
v = ( 0.24 * 8.314 * 273 ) / 1 atm
= 544.7 ml = 5.4 L
Hence we can conclude that The volume of carbon dioxide produced is : 5.4 L
Learn more about Propane burning at STP : brainly.com/question/11903456
Answer:
Yes
Explanation:
: The corrosion of iron indicates a chemical change in the metal. ... Where salt is present, electrochemical corrosion occurs, and the protective oxide film does not form, thus the corrosion (buildup of rust) continues unchecked. Your iron nail will indeed rust more quickly and severely in salt water.
Answer:
Pressure of neon = 1.17 atm
Pressure of hydrogen = 0.63 atm
Explanation:
Given data:
Number of moles of H₂ = 2.5 mol
Number of moles of Ne = 4.6 mol
Total pressure = 1400 mmHg (1400/760 = 1.8 atm)
Solution:
We will solve this problem through mole fraction method.
Total number of moles = 2.5 + 4.6 = 7.1
Mole fraction of H₂ Mole fraction of Ne
2.5 mol/7.1 mol= 0.35 4.6mol/7.1mol = 0.65
Pressure of hydrogen = 0.35 × 1.8 atm
Pressure of hydrogen = 0.63 atm
Pressure of neon = 0.65 × 1.8 atm
Pressure of neon = 1.17 atm
Total pressure which is already given is sum of partial pressure of hydrogen and neon gas.
0.63 atm + 1.17 atm = 1.8 atm