Answer:
Bin 1 points to a carbon bonded to a double bonded carbon and single bonded to two hydrogens. --- trigonal planar, tetrahedral
Bin 2 points to a carbon double bonded to a carbon and single bonded to a carbon and one hydrogen.------- trigonal planar, tetrahedral
Bin 3 is a carbon single bonded to two carbons and single bonded to two hydrogens. ----- tetrahedral, tetrahedral
Bin 4 is the same as bin 3.--------tetrahedral, tetrahedral
Bin 5 is a carbon triple bonded to a carbon and single bonded to a carbon.---- linear, tetrahedral
Bin 6 is triple bonded to a carbon and single bonded to a hydrogen.---linear, tetrahedral
Explanation:
A single C-C or C-H bond is in a tetrahedral geometry, the carbon atom is bonded to four species with a bond angle of 109°.
A C=C bond is trigonal planar with a bond angle of 120°.
Lastly, a C≡C bond has a linear geometry with a bond angle of 180° between the atoms of the bond.
Considering ideal gas behavior, the volume of 1 mol of gas at STP is 22.4 L; then the volume occupied by 1.9 moles is 1.9mol*22.4L/mol
The answer is 43 L if I am correct.
The answer is True because they are formed of deposition.
The empirical formula is the lowest reduced ration of the atoms present. In this case, it is P2O5
Answer:
5.19 m³
Explanation:
Data Given:
initial Pressure P1 = atmospheric pressure
Reported atmospheric pressure = 14.696 psi
Final pressures P2 = 68 psi
initial Temperature T1 = 26 °C
final Temperature T2 = 48 °C
initial Volume V1= 13 m³
final Volume V2 = ?
Solution:
Formula will be used
P1 V1 / T1 = P2 V2 / T2
To calculate volume rearrange the above formula
V2 = (P1 V1) T2 / T1 P2 . . . . . . . .(1)
put values in equation 1
V2 = (14.696 psi x 13 m³) 48 °C / 26 °C x 68 psi
V2 = (191.05 psi m³) 48 °C / 1768 °C psi
V2 = (9170.3 psi m³ °C / 1768 °C psi
V2 = 5.19 m³
So, final volume is 5.19 m³
