Answer:
Sr would be the limiting reactant
5 moles
Explanation:
Since the equation is a balanced equation, the coefficient shows how each substance relates to the other in terms of the number of moles.
Reactants would be those on the left hand side of the arrow, while the products would be found on te right and side of the arrow. In this question, the reactants would be Sr and O₂.
Limiting reactant is the reactant that is insufficient; meaning to say that there is not enough of that substance and thus the reaction cannot continue. The other reactant(s) that is not limiting is called the excess reactants.
From the balanced equation, 2 moles of Sr is needed to react with 1 mole of O₂. Thus, if we have 5 moles of each reactant, Sr would be the limiting reactant since for every 1 mole of O₂, there has to be 2 moles of Sr in order for the reaction to proceed. Thus, if we have 5 moles of O₂, we would need 10 moles of Sr.
When we work out the amount of products formed, we look at the number of moles of the limiting reactant. This is because the limiting reactant determines how much is being reacted, while the excess number of moles of the excess reactant will remain unreacted.
For every 2 moles of Sr reacted, 2 moles of SrO would be produced. This means that the mole ratio of Sr to SrO is 1:1. Thus, since 5 moles of Sr has been reacted, 5 moles of the product (SrO) would be produced.
Answer:
pH = 7.8
Explanation:
The Henderson-Hasselbalch equation may be used to solve the problem:
pH = pKa + log([A⁻] / [HA])
The solution of concentration 0.001 M is a formal concentration, which means that it is the sum of the concentrations of the different forms of the acid. In order to find the concentration of the deprotonated form, the following equation is used:
[HA] + [A⁻] = 0.001 M
[A⁻] = 0.001 M - 0.0002 M = 0.0008 M
The values can then be substituted into the Henderson-Hasselbalch equation:
pH = 7.2 + log(0.0008M/0.0002M) = 7.8
Due to it's electronic configuration w/c is 1s2 2s2 2ps 3s1 considering the last w/c is 3s1, sodium should be in row 3 period a1.
Answer:
1.25 atm.
Explanation:
Step 1:
Data obtained from the question. This includes the following:
Initial volume (V1) = 20L
Initial temperature (T1) = 25°C
Initial pressure = 1 atm
Final temperature (T2) = 100°C
Final volume (V2) = constant i.e remain the same
Final pressure (P2) =?
Step 2:
Conversion of celsius temperature to Kelvin temperature. This is illustrated below:
Temperature (Kelvin) = temperature (celsius) + 273
Initial temperature (T1) = 25°C = 25°C + 273 = 298K
Final temperature (T2) = 100°C = 100°C + 273 = 373K
Step 3:
Determination of the final pressure of the gas. This is illustrated below:
Since the volume is constant, the following equation, P1/T1 = P2/T2 will be used to obtain the final pressure of gas as follow:
P1/T1 = P2/T2
Initial temperature (T1) = 298k
Initial pressure = 1 atm
Final temperature (T2) = 373K
Final pressure (P2) =?
P1/T1 = P2/T2
1/298 = P2 /373
Cross multiply to express in linear form
298 x P2 = 1 x 373
Divide both side by 298
P2 = 373/298
P2 = 1.25 atm.
Therefore, the pressure of the heated gas is 1.25 atm.
Answer:
Explanation:
Moles of SO₃ = 0.760 mol
Volume = 1.50 L
[SO₃] = 0.5067 M
Considering the ICE table for the equilibrium as:
Given:
Equilibrium concentration of O₂ = 0.130 mol
Volume = 1.50 L
[O₂] = x = 0.0867 M
[SO₂] = 2x = 0.1733 M
[SO₃] = 0.5067-2x = 0.3334 M
The expression for the equilibrium constant is:
![K_c=\frac {[SO_2]^2[O_2]}{[SO_3]^2}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%20%7B%5BSO_2%5D%5E2%5BO_2%5D%7D%7B%5BSO_3%5D%5E2%7D)
