To solve this kinematics formula use the following equation:
Vf = Vi + at
Vf = 0 + (9.81 m/s^2)(3 seconds)
Vf = 29.43 m/s and or about 29.4 m/s of reported to 3 significant figures.
The above question is incomplete, here is the complete question:
Calculate the standard molar enthalpy of formation of NO(g) from the following data at 298 K:
![N_2(g) + 2O_2 \rightarrow 2NO_2(g), \Delta H^o = 66.4 kJ](https://tex.z-dn.net/?f=N_2%28g%29%20%2B%202O_2%20%5Crightarrow%202NO_2%28g%29%2C%20%5CDelta%20H%5Eo%20%3D%2066.4%20kJ)
![2NO(g) + O_2\rightarrow 2NO_2(g),\Delta H^o= -114.1 kJ](https://tex.z-dn.net/?f=2NO%28g%29%20%2B%20O_2%5Crightarrow%202NO_2%28g%29%2C%5CDelta%20H%5Eo%3D%20-114.1%20kJ)
Answer:
The standard molar enthalpy of formation of NO is 90.25 kJ/mol.
Explanation:
![N_2(g) + 2O_2 \rightarrow 2NO_2(g), \Delta H^o_{1} = 66.4 kJ](https://tex.z-dn.net/?f=N_2%28g%29%20%2B%202O_2%20%5Crightarrow%202NO_2%28g%29%2C%20%5CDelta%20H%5Eo_%7B1%7D%20%3D%2066.4%20kJ)
![2NO(g) + O_2\rightarrow 2NO_2(g),\Delta H^o_{2} = -114.1 kJ](https://tex.z-dn.net/?f=2NO%28g%29%20%2B%20O_2%5Crightarrow%202NO_2%28g%29%2C%5CDelta%20H%5Eo_%7B2%7D%20%3D%20-114.1%20kJ)
To calculate the standard molar enthalpy of formation
...[3]
Using Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.
[1] - [2] = [3]
![N_2+O_2\rightarrow 2NO(g),\Delta H^o_{3} = ?](https://tex.z-dn.net/?f=N_2%2BO_2%5Crightarrow%202NO%28g%29%2C%5CDelta%20H%5Eo_%7B3%7D%20%3D%20%3F)
![\Delta H^o_{3} =\Delta H^o_{1} - \Delta H^o_{2}](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7B3%7D%20%3D%5CDelta%20H%5Eo_%7B1%7D%20-%20%5CDelta%20H%5Eo_%7B2%7D%20)
![\Delta H^o_{3}=66.4 kJ - [ -114.1 kJ] = 180.5 kJ](https://tex.z-dn.net/?f=%5CDelta%20H%5Eo_%7B3%7D%3D66.4%20kJ%20-%20%5B%20-114.1%20kJ%5D%20%3D%20180.5%20kJ)
According to reaction [3], 1 mole of nitrogen gas and 1 mole of oxygen gas gives 2 mole of nitrogen monoxide, So, the standard molar enthalpy of formation of 1 mole of NO gas :
=![\frac{\Delta H^o_{3}}{2 mol}](https://tex.z-dn.net/?f=%5Cfrac%7B%5CDelta%20H%5Eo_%7B3%7D%7D%7B2%20mol%7D)
![=\frac{180.5 kJ}{2 mol}=90.25 kJ/mol](https://tex.z-dn.net/?f=%3D%5Cfrac%7B180.5%20kJ%7D%7B2%20mol%7D%3D90.25%20kJ%2Fmol)
D.
Gastropods live in every conceivable habitat
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