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3 years ago

Give an example of a state function and explain why it is a state function

Chemistry

1 answer:

inessss [21]3 years ago

4 0

A specific state which is defined being a property without the path taken to achieve that state based on it, is understood as a state function.
While the functions whose value is based on the direction taken among two states are named direction or path functions, on the other hand.
The system's thermodynamic condition relates to the current material in temperature, pressure and quantity.
State functions rely only on certain requirements and not on how they have been achieved. State functions for an instance, involve entropy, density, enthalpy and internal energy.
They are known as state functions as they quantitatively define a thermodynamic system's equilibrium condition, regardless of how the system landed in that condition.

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What is the formula for Boron TriHydride?

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I got BH3, but just letting you know I am 97% sure on that. I hope it helps!!

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3 years ago

According to the law of conservation of mass, the total mass of the reactants is

yarga [219]

Answer:

is equal to the total number of products

Explanation:

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3 years ago

How many moles of oxygen atoms are in 7.9E-1 moles of CO_2

Ilya [14]

Answer:

The number of moles of O atom in $(7.9\times10^{-1})$ mol of $CO_{2}$ = 1.6

Explanation:

1 molecule of $CO_{2}$ contains 2 atoms of O

So, $(6.023\times 10^{23})$ molecules of $CO_{2}$ contains $(2\times6.023\times10^{23})$ atoms of O.

We know that 1 mol of an atom/molecule/ion represents $6.023\times10^{23}$ numbers of atoms/molecules/ions respectively.

So, $(6.023\times 10^{23})$ molecules of $CO_{2}$ is equal to 1 mol of $CO_{2}$ .

$(2\times6.023\times10^{23})$ atoms of O is equal to 2 moles of O atom.

Hence, 1 mol of $CO_{2}$ contains 2 moles of O atom.

Therefore, $(7.9\times10^{-1})$ mol of $CO_{2}$ contains $(2\times7.9\times10^{-1})$ moles of O atom or 1.6 moles of O atom.

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3 years ago

How many grams of NH4ClO4 would dissolve in 250 mL at 30 C

baherus [9]

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3 years ago

Determine the enthalpy of neutralization in Joules/mmol for a solution resulting from 19 mL of 0.9 M NaOH solution and 19 mL of

Rina8888 [55]

Answer:

3.00 J/mmol

Explanation:

The temperature of the solution is increasing, so it's an endothermic reaction. The heat that is being absorbed can be calculated by:

Q = m*c*ΔT

Where m is the total mass (HCl + NaOH), c is the specific heat, and ΔT is the variation of the temperature (final - initial). Because the molarity is small, the solutions are basically water, so c = 4.184 J/g°C.

The mass is the molar mass multiplied by the number of moles (n), which is the volume multiplied by the molarity:

nHCl = 0.9 mol/L *0.019 = 0.0171 mol

nNaOH = 0.9 mol/L *0.019 = 0.0171 mol

Molar masses: HCl = 36.5 g/mol; NaOH = 40 g/mol

mHCl = 36.5*0.0171 = 0.62415 g

mNaOH = 40 * 0.0171 = 0.6840 g

m = 1.30815 g

Q = 1.30815*4.184*(37.8 - 28.8)

Q = 49.2597 J

Because the number of moles of NaOH is equal to the number of moles of HCl, and the stoichiometry of the neutralization is 1:1, they both react completely, so the enthalpy can be calculated based in any of them. The enthalpy is the heat divided by the number of moles. In mmol, n is 17.1 mmol.

ΔH = 49.2597/17.1

ΔH = 2.88 J/mmol

ΔH = 3.00 J/mmol

7 0

3 years ago