Answer:
569K
Explanation:
Q = 3.5kJ = 3500J
mass = 28.2g
∅1 = 20°C = 20 + 273 = 293K
∅2 = x
c = 0.449
Q = mc∆∅
3500 = 28.2×0.449×∆∅
3500 = 12.6618×∆∅
∆∅ = 3500/12.6618
∆∅ = 276.4220
∅2 - ∅1 = 276.4220
∅2 = 276.4220 + ∅1
∅2 = 276.4220 + 293
∅2 = 569.4220K
∅2 = 569K
Answer:
Ethanol has covalent intramolecular bonds. Ethanol is polar. Ethanol has dispersion intermolecular forces. Dimethyl ether is polar. Dimethyl ether forms hydrogen bonds. Dimethyl ether has dispersion intermolecular forces.
Explanation:
Ethanol is not a carboxylic acid. It is an alcohol and it has covelent intramolecular bonds. It is polar and it also has dispersion intermolecular forces.
Dimethyl ether is also polar and it has forms hydrogen bonds. It also has dispersion intermolecular forces. Dimethyl ether does not have ionic intramolecular forces
Explanation:
Expression for the 
speed is as follows.
where, = root mean square speed
k = Boltzmann constant
T = temperature
M = molecular mass
As the molecular weight of oxygen is 0.031 kg/mol and R = 8.314 J/mol K. Hence, we will calculate the value of as follows.
= 
= 498.5 m/s
Hence, for oxygen atom is 498.5 m/s.
For nitrogen atom, the molecular weight is 0.028 kg/mol. Hence, we will calculate its speed as follows.
= 
= 524.5 m/s
Therefore, speed for nitrogen is 524.5 m/s.
Molar mass
C₂H₄O₂ = 60.0 g/mol
n = mass / molar mass
3.00 = mass / 60.0
m = 3.00 * 60.0
m = 180 g of <span>C₂H₄O₂
hope this helps!</span>
Answer:
The answer to your question is: ΔH = -283 kJ/mol, first option
Explanation:
Reaction
CO + O₂ ⇒ CO₂
ΔH = ∑H products - ∑H products
ΔH = -393.5 - (-110.5 + 0)
ΔH = -393.5 + 110.5
ΔH = -283 kJ/mol
