Depending on how the design is, The bridge will sway, bounce, or move in some way. If the bridge was too stiff the winds would destroy the bridge and cause it to crumble and fall.
Hope that answer works for you! :)
Answer:
ΔG° of reaction = -47.3 x 
J/mol
Explanation:
As we can see, we have been a particular reaction and Energy values as well.
ΔG° of reaction = -30.5 kJ/mol
Temperature = 37°C.
And we have to calculat the ΔG° of reaction in the biological cell which contains ATP, ADP and HPO4-2:
The first step is to calculate the equilibrium constant for the reaction:
Equilibrium Constant K = ![\frac{[HPO4-2] x [ADP]}{ATP}](https://tex.z-dn.net/?f=%5Cfrac%7B%5BHPO4-2%5D%20x%20%5BADP%5D%7D%7BATP%7D)
And we have values given for these quantities in the biological cell:
[HP04-2] = 2.1 x 
M
[ATP] = 1.2 x 
M
[ADP] = 8.4 x M
Let's plug in these values in the above equation for equilibrium constant:
K = ![\frac{[2.1x10^{-3}] x [8.4x10^{-3}] }{[1.2 x 10^{-2}] }](https://tex.z-dn.net/?f=%5Cfrac%7B%5B2.1x10%5E%7B-3%7D%5D%20x%20%5B8.4x10%5E%7B-3%7D%5D%20%7D%7B%5B1.2%20x%2010%5E%7B-2%7D%5D%20%7D)
K = 1.47 x M
Now, we have to calculate the ΔG° of reaction for the biological cell:
But first we have to convert the temperature in Kelvin scale.
Temp = 37°C
Temp = 37 + 273
Temp = 310 K
ΔG° of reaction = (-30.5 ) + (8.314)x (310K)xln(0.00147)
Where 8.314 = value of Gas Constant
ΔG° of reaction = (-30.5 x ) + (-16810.68)
ΔG° of reaction = -47.3 x J/mol
Answer/Explanation:
Aluminum and oxygen
Fluorine and oxygen
Ionic compounds are formed when any type of metal is combined with a non-metal such as carbon, nitrogen, oxygen, sulfur, phosphorus, and selenium.
(any)metal + nonmetal = ionic compound
It will likely give up its valence electron to the other compound, forming stable octets on each of the newly formed ions. These ions have opposing charges, and tend to form strong ionic lattices. A good example of this is NaCl, which contains Na+ ions that have given up their one valence electron and Cl- ions which have accepted that electron.
Hope this helps!
Answer:
Mass of CO₂ produced = 5.72 g
Explanation:
Given data:
Mass of methane = 2.34 g
Mass of oxygen = 8.32 g
Mass of CO₂ produced = ?
Solution:
Chemical equation:
CH₄ + 2O₂ → CO₂ + 2H₂O
Number of moles of methane:
Number of moles = mass/molar mass
Number of moles = 2.34 g/ 16 g/mol
Number of moles = 0.146 mol
Number of moles of oxygen:
Number of moles = mass/molar mass
Number of moles = 8.32 g/ 32 g/mol
Number of moles = 0.26 mol
Now we will compare the moles of carbon dioxide with oxygen and methane.
CH₄ : CO₂
1 : 1
0.146 : 0.146
O₂ : CO₂
2 : 1
0.26 : 1/2×0.26 = 0.13 mol
Less number of moles of CO₂ are produced by oxygen thus oxygen will react as limiting reactant.
Mass of CO₂:
Mass = number of moles × molar mass
Mass = 0.13 mol × 44 g/mol
Mass = 5.72 g
