It follows that the reaction is spontaneous at high temperatures Option A.
<h3>What is ΔS ?</h3>
The term ΔS is referred to as the change in the entropy of the system. Now recall that entropy is defined as the degree of disorderliness in a system. If a system is highly disorderly then it means that it has a high entropy. Also, ΔH has to do with the heat change that accompanies a reaction.
We know that both the entropy and the heat change can both either be positive or negative. Now we know that the equation ΔG = ΔH - TΔS can be used to ascertain whether or not a reaction will be spontaneous. If the result is negative, then the reaction will be spontaneous.
As such, when then it follows that the reaction is spontaneous at high temperatures Option A.
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Answer:
Whether the mixture can be separated
Answer:
There are 120 possible ways.To calculate the number of permutations here, where order is important and repetition is not allowed, we use the following formula:Number of permutations = n! / (n - r)! = 5!/0! = 12345 / 1 (note: "!" means "factorial" and 0! equals 1) = 120/1 = 120.For a complete list see below. Let a,b,c,d & e represent the 5 players and their order determine their position:{a,b,c,d,e}
Explanation:
6.4 x 10^-7 = [CO]^2[O2]/ [CO2}^2 = ( 2.0 x 10^-3)^2 ( 1.0 x 10^-3)/ [CO2]^2 =
<span>=4.0 x 10^-9 / [CO2]^2 </span>
<span>[CO]= sq.rt ( 4.0 x 10^-9)/ 6.4 x 10^-7=7.9 x 10^-2 M </span>
<span>2.6 x 10^-3 = [I]^2 / [I2] = [I]^2 / 0.95 </span>
<span>[I]= sq.rt ( 2.6 x 10^-3 x 0.95)=5.0 x 10^-2 M </span>
<span>Ksp = [Ba2+][CO32-] = ( 1.1 x 10^-4)^2=1.2 x 10^-8</span>
It's very simple... if we remember value of Universal Gas Constant R and Ideal Gas Law, so...
Ideal Gas Law
pV = nRT, where:
p - pressure (in kPa),
V - volume (in L),
n - number of moles (in mol),
R - universal cas constant (in kPa * L / mo l* K),
T - temperature (in K)
n = m/M, where:
n - number of moles,
m - mass (in grams),
M - molar mass of ingredient (in g/mol) - you find this at Periodic Table.
pV = nRT ---> pV = mRT/M ---> pVM = mRT ---> pVM/RT = m
p = 17615 kPa
T = 273.15 + 23 = 296.15 K
V = 43.8 L
R = 8.314 kPa * L / mol * K
M (for argon) = 39.948 g/mol
and
m = (17615 kPa * 48.3 L * 39.948 g/mol) / (296.15 K * 8.314 kPa * L / mol * K)
m = 13803.93 grams of Argon
