# Given these reactions, X ( s ) + 1 2 O 2 ( g ) ⟶ XO ( s ) Δ H = − 668.5 k J / m o l XCO 3 ( s ) ⟶ XO ( s ) + CO 2 ( g ) Δ H = + 384.3 k J / m o l what is Δ H for this reaction? X ( s ) + 1 2 O 2 ( g ) + CO 2 ( g ) ⟶ XCO 3 ( s )

Answer: The for the reaction is -1052.8 kJ.

Explanation:

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.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

The intermediate balanced chemical reaction are:

(1)

(2)

The expression for enthalpy of the reaction follows:

Putting values in above equation, we get:

Hence, the for the reaction is -1052.8 kJ.

## Related Questions

A solution is dilute when?A. it has a lot of solute
B. has little solvent
C. it has a lot of solvent
D. has maximum solute

C. It has more solvent
To dilute a solution means to add more solvent without the addition of more solute

I AM STRESSED AS WELL

Sodium phosphate and calcium chloride react to form sodium chloride and calcium phosphate. If you have 379.4 grams of calcium chloride and an excess of sodium phosphate, how much calcium phosphate can you make?

Solution:- The balanced equation is:

We start with given grams of calcium chloride and convert them to moles. Then using mol ratio, the moles of calcium phosphate are calculated and converted to grams as.

Molar mass of calcium chloride is 110.98 gram per mol and molar mass of calcium phosphate is 310 gram per mol.

The set is made using dimensional analysis as:

=

So, 353.3 grams of calcium phosphate can be formed.

353.3g

Explanation:

How to prepare ethanoic acid from ethane

anonymous
anonymous 5 years ago
First you chlorinate it in presence of light.
C2H6 + Cl2 ---hv -> C2H5Cl + HCl
Then you add aqeuos KOH to get C2H5OH
C2H5Cl+KOH-> C2H5OH+ KCl.
Then you add KMnO4 to get the rquired compound.
C2H5OH ----KMnO4 ---> CH3COOH.
C2h6 + O2 ----> CH3CooH

At standard temperature and pressure (0 ∘C and 1.00 atm ), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 55 ∘C ?

Taking into account the Charles's law, the same amount of gas at the same pressure and 55 ∘C would occupy a volume of 26.91 L.

Charles's Law consists of the relationship that exists between the volume and the temperature of a certain quantity of ideal gas, which is maintained at a constant pressure.

This law states that the volume is directly proportional to the temperature of the gas: if the temperature increases, the volume of the gas increases, while if the temperature of the gas decreases, the volume decreases.

Mathematically, Charles's law is a law that says that when the amount of gas and pressure are kept constant, the quotient that exists between the volume and the temperature will always have the same value:

Studying an initial state 1 and a final state 2, it is satisfied:

In this case, you know:

• V1= 22.4 L
• T1= 0 C= 273 K
• V2= ?
• T2= 55 C= 328 K

Replacing:

Solving:

V2= 26.91 L

Finally, the same amount of gas at the same pressure and 55 ∘C would occupy a volume of 26.91 L.

Explanation: this is Charles' law which states that the volume of a gas is directly proportional to the absolute temperature at contant pressure. The expression is V1/T1 = V2/T2

Making V2 the subject of the formula we have

V2 = V1 xT2/T1

= 22.4 x 328/273

= 26.9L

Convert 50g of calcium carbonate, CaCO3, into moles

Moles  =  0.5 mol

Solution:

Moles is related to mass as follow,

Moles  =  Mass / M.mass   ----- (1)

Where;
Mass  =  50 g

M.mass  =  Ca (40) + C (12) + O₃ (16)₃  =  100 g/mol

Putting values in equation 1,

Moles  =  50 g ÷ 100 g.mol⁻¹

Moles  =  0.5 mol