The mass of Iron produced by the reaction of given reactants will be 64.3 grams.
The balanced reaction is given as,
Fe₂O₃ + 3CO= 2Fe + 3CO₂
According to the chemical equation, 3 moles of carbon monoxide, CO, will react with 1mole of ferric oxide, Fe₂O₃, and produce 3 moles of carbon dioxide, CO₂
Now, we are given moles of carbon monoxide and asked for moles of Iron. This means that we will have to convert the aforementioned mole ratio that exists between carbon monoxide and carbon dioxide to a gram ratio.
If one mole of Iron has the mass of 55.845 g and one mole of carbon dioxide has a mass of 44.01 g, it follows that reaction produces
44.01g of carbon dioxide for the every 55.845 g of Iron.
So for 1 moles of carbon dioxide the mass will be 44.01 g
For 3 moles it is 3× 44.01 =132.03 gram
1 mole carbon dioxide has 55.845 g iron
0.576 moles has 55.845×0.576
44.01×3 g of carbon dioxide = 132.03 g
55.845×2 g of Iron = 111.69 g
So in 0.576 moles it will get 111.69×0.576
=64.3 grams of Iron are produced.
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A chemical formula of an unknown metal (M) combines with chlorine in the followingformula:MC15What is the charge of the metal
Answer:
The charge of the metal is +5.
Explanation:
As the chlorine atom has a valence of -1, and the metals have a positive valence, we have to look for the charge that makes the molecule neutral.
In this case, there are 5 Cl, so the total negative charge of Cl is -5.
To make the molecule neutral, the metal must have a positive charge of +5.
Write a net ionic equation for this reaction.Express your answer as a chemical equation. Identify all of the phases in your answer.ANSWER:
Given the reaction:
[tex]2HNO_3+Ca(OH)_2\to Ca(NO_3)_2+2H_2O[/tex]We're going to write a net ionic equation for this reaction as follows:
1. First, write the total ionic equation:
[tex]^{}Ca^{2+}_{aq}+2OH^-_{aq}+2H^+_{aq_{}}+2NO^-_3\to^{}Ca^{2+}_{aq}+2NO^-_3+2H_2O[/tex]2. Now, we could cancel the same type of ions that are in both sides of the reaction. Therefore, the net ionic equation is:
[tex]H^+_{aq}+^{}OH^-_{aq}\to H_2O_{(l)}[/tex]Convert 960 Torr to kPa
Step 1
Torr and kPa are units of pressure
---------
Step 2
The equivalence:
760 torr = 101325 Pa
1 kPa = 1000 Pa
Procedure:
960 Torr x (101325 Pa/760 Torr) = 127989.47 Pa
Then, 127989.47 Pa x (1 kPa/1000 Pa) = 128 kPa approx.
Answer: Pressure = 128 kPa
16. Which of the following is directly responsible for acid rain? A. steam vented from a nuclear power plant B. sulfur dioxide released from a coal-fired power plant. C. mining of coal for a coal-fired power plant D. processing of uranium for a nuclear power plant
Answer
B. sulfur dioxide released from a coal-fired power plant.
Explanation
Power plants release the majority of sulfur dioxide and much of the nitrogen oxides when they burn fossil fuels, such as coal, to produce electricity. In addition, the exhaust from cars, trucks, and buses releases nitrogen oxides and sulfur dioxide into the air. These pollutants cause acid rain.
Therefore, what is directly responsible for acid rain is:
B. sulfur dioxide released from a coal-fired power plant.
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Rb+
Fe2+
H-
Al3+
Cl-
O2-
Using the ions above, write the formulas and give the names for 5 possible ionic compounds involving these ions.
The formulas and and the names for 5 possible ionic compounds involving these ions are :
Rb₂O, Rubidium Oxide
FeCl₂, Iron(II)chloride
Al(OH)₃ , Aluminum hydroxide
LiH, Lithium Hydride
NaCl, Sodium chloride
1) The Rb₂O is called as Rubidium oxide. rubidium oxide is an ionic compound. Ionic compound formed between a positive ion called cation and a negative ion called anion . ionic bond is formed with the complete transfer of electrons. In Rubidium oxide : the cation is Rb⁺ and the anion is O²⁻.
2) The FeCl₂ is called as iron(II)chloride. iron(II)chloride is an ionic compound. in iron(II)chloride : the cation is Fe²⁺ and the anion is Cl⁻.
3) Al(OH)₃ is aluminum hydroxide . In aluminum hydroxide : the cation is present as Al³⁺ and anion is present as OH⁻.
4) LiH is lithium hydride . the cation is Li⁺ and the anion is H⁻.
5) NaCl is sodium chloride. cation is Na⁺ and anion is Cl⁻
Thus, The formulas and and the names for 5 possible ionic compounds involving these ions. Rb₂O, Rubidium Oxide
FeCl₂, Iron(II)chloride
Al(OH)₃ , Aluminum hydroxide
LiH, Lithium Hydride
NaCl, Sodium chloride
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What is the charge on a sulfur atom that contains 18e−e−?
Sulphur atom has 16 as its atomic number, which is also the same number of protons and the same number of electrons:
Z = 16
P = 16
e- = 16
But when we have a Sulphur ion, it is usually -2, and since we have 18 electrons in this case, the charge will be -2
Which of the following are organic compounds? (a). CH3CH3 (b). NH3 (c). CH3SCH3 (d). CH3CH2OH (e). Mg(OH)2
CH3CH3
CH3SCH3
CH3CH2OH
Explanations;What are organic compounds?
Organic compounds are compounds that class of compounds that contains the carbon-hydrogen bond. This means that for a compound to be classified as an organic compound, they must contain the C-H bond in their compound
From the listed compouds, the compound that contains theC-H bonds are:
• CH3CH3
,• CH3SCH3
,• CH3CH2OH
These are therefore considered the required list of organic compounds from the given options
Calculate the molarity of a solution that contains 0.75 mol of KCI in 0.250L of solution
The molarity of a solution that contains 0.75 mol of KCI in 0.250L of the solution is 3 M
The number of moles per liter of solution is termed molarity.
M=n/V(in L)
M is the molarity
n is the number of moles
V is the volume
Substituting the values, we get
M=0.75/0.25=3
The molarity is 3 M
Molarity is a concentration term and denotes the number of moles dissolved per liter.It can be defined as the amount of substance in a particular volume of solution.The unit is mol/LIt can be found by the given mass and volume of the solution.To learn more about molarity visit:
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A testing chamber holds a 2.50 L sample of neon gas at 325.0 K.If the pressure is measured inside the chamber as 4.00 atm, how many moles of neon are present?0.4530.44200.3750.326
Answer: There are 0.375 moles of neon gas present in the testing chamber.
Explanation:
The question requires us to calculate the number of moles of neon gas, given that the gas is in a 2.50 L chamber at 325.0 K and the pressure inside the chamber is 4.00 atm.
We can solve this problem using the equation for ideal gases, as shown below:
[tex]PV=nRT[/tex]where P is the pressure of the gas (P = 4.00 atm), V is the volume of the gas (V = 2.50 L), n is the number of moles, that we want to calculate, T is the temperature of the gas (T = 325.0 K) and R is the gas constant.
Note that the values of pressure and volume are given in atm and L, respectively. Therefore, we can apply the gas constant in units of L.atm/mol.K:
R = 0.082057 L.atm/K.mol
First, let's rearrange the equation of ideal gases in order to calculate the number of moles of gas:
[tex]PV=nRT\rightarrow n=\frac{PV}{RT}[/tex]Now, applying the values given by the question and the constant R, we'll have:
[tex]n=\frac{(4.00atm)\times(2.50L)}{(0.082057L.atm/K.mol)\times(325.0K)}=0.375mol[/tex]Therefore, there are 0.375 moles of neon gas in the testing chamber under the conditions given by the question.
Force and distance are used to calculate work. Work is measured in which unit?
Answer: Joules (J)
Explanation:
Answer:
Joules or Newton metre
Explanation:
Work = Force × distance
Force = kgm/s² (Newton)
×
Distance = m
= kgm²/s² (Newton metre or Joules) (Nm or J)
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A single bond is made up of 1.0 sigma bond and no pi bonds.
Pi bonds appears from double bonds onwards.
5. What is the amount of moles of nitrous oxide gas (N2O) used to sedate Mr. Muthbefore his wisdom teeth are pulled? The pressure is 2.5 atm, a temperature of 25.and volume of 1.67L?tbd
Step 1 - Understanding how mole relates to temperature, pressure and volume
These variables are related according to the ideal gas equation:
[tex]pV=nRT[/tex]We can use this equation to predict the behavior as well as the quantity of a gas, given that the remaining variables are given.
Step 2 - Using the equation to solve the equation
According to the exercise:
[tex]\begin{gathered} p=2.5atm \\ T=25°C\text{ \lparen298 K\rparen} \\ V=1.67L \\ n=? \end{gathered}[/tex]Setting the values in the equation:
[tex]2.5\times1.67=nR\times298[/tex]We need to make two observations now: the temperature must be in Kelvin in this equation for it to work. R stands for the universal gas constant, as has the value of 0.082 atm.L/mol.K.
Therefore:
[tex]\begin{gathered} 2.5\times1.67=n\times0.082\times300 \\ \\ n=\frac{4.17}{24.6}=0.169\approx0.17 \end{gathered}[/tex]Answer: the amount of moles used is 0.17 moles.
2C2H2 + 5O2 —> 4CO2 + 2H2OIf 3.80 moles of oxygen wre used up in the reaction, how many moles of water are produced?
In order to solve this question, we can use the concept of molar ratio, which means the amount of reactant is needed in order to produce a certain amount of product. In our question we have:
2 C2H2 + 5 O2 -> 4 CO2 + 2 H2O
The molar ratio between O2 and H2O is 5:2 (we use only the numbers in front of the compound), so that means that for every 5 moles of O2 used, we will have 2 moles of H2O being produce, now we can use this information to calculate how many moles of H2O will be produced from 3.80 moles of O2
5 O2 = 2 H2O
3.80 O2 = x H2O
x = 1.52 moles of H2O are produced from 3.80 moles of O2
Calculate how many grams of MgCl2 are needed to produce 12.15 grams
Answer
47.60 g
Explanation
Given that:
Molar mass of MgCl₂ = 95.20 g/mol
Mass of Mg produced = 12.15 grams
Equation: MgCl₂ → Mg + Cl₂
What to find:
To calculate the grams of MgCl₂ needed to produce 12.15 grams of Mg.
Step-by-step solution:
Step 1: Convert the mass of Mg produced to moles.
Using the molar mass of Mg (24.305 g/mol) and the mole formula, the moles of Mg produced is
[tex]Moles=\frac{mass}{molar\text{ }mass}=\frac{12.15\text{ }g}{24.305\text{ }g\text{/}mol}=0.49989714\text{ }mol[/tex]Step 2: Determine the moles of MgCl₂ needed to produce 12.15 g of Mg.
According to the given equation; 1 mol of MgCl₂ produced 1 mol of Mg
So, x mol of MgCl₂ will produce 0.49989714 mol of Mg
That is:
[tex]\begin{gathered} 1mol\text{ }MgCl₂=1mol\text{ }Mg \\ \\ x=0.49989714mol\text{ }Mg \\ \\ x=\frac{0.49989714mol\text{ }Mg}{1mol\text{ }Mg}\times1mol\text{ }MgCl₂ \\ \\ x=0.49989714mol\text{ }MgCl₂ \end{gathered}[/tex]Step 3: Convert the moles of MgCl₂ needed to produce 12.15 g of Mg to grams.
Using the molar mass of MgCl₂ = 95.20 g/mol, therefore the mass in grams of MgCl₂ needed to produce 12.15 g of Mg will be:
[tex]\begin{gathered} Mass\text{ }of\text{ }MgCl_2\text{ }needed=Molar\text{ }mass\times Moles \\ \\ Mass\text{ }of\text{ }MgCl_2\text{ }needed=95.20\text{ }g\text{/}mol\times0.49989714\text{ }mol \\ \\ Mass\text{ }of\text{ }MgCl_2\text{ }needed=47.60\text{ }g \end{gathered}[/tex]Hence, the grams of MgCl₂ needed to produce 12.15 grams of Mg is 47.60 g.
How many moles in 2.24 L of a sample of gas.1 mol10 mole0.1 mole5 mol
Answer:
[tex]0.1\text{ mole}[/tex]Explanation:
Here, we want to get the number of moles in 2.24 L of a sample of gas
Mathematically,
At STP, 1 mole of a gas occupies a volume of 22.4 L
Thus x moles will occupy 2.24 L at STP
To get the value of x, we have it that:
[tex]\begin{gathered} x\times22.4\text{ = 1}\times2.24 \\ x\text{ = }\frac{2.24}{22.4} \\ \\ x\text{ = 0.1 mole} \end{gathered}[/tex]4 N2H3CH3 (l) + 5 N2O4 (l) →12 H2O(g) + 9 N2(g) + 4 CO2 (g)The enthalpy of formation for liquid methylhydrazine is +53 kJ/mol and the enthalpy of formation for liquid dinitrogen tetroxide is -20 kJ/mol. Calculate ∆H° for this reaction, ignore significant digits for this question.
Answer
[tex]\Delta H_{rxn}\operatorname{\degree}=-4791.6\text{ }kJ\text{/}mol[/tex]Explanation
The given chemical equation for the reaction is:
[tex]4N_2H_3CH_3(l)+5N_2O_4(l)\text{ }→\text{ }12H_2O\left(g\right)+9N_2\left(g\right)+4CO_2(g)[/tex]From the given table and question, the enthalpies of formation of the reactants ad products are:
[tex]\begin{gathered} ∆H_f°(N_2H_3CH_{3(l)})=+53\text{ }kJ\text{/}mol \\ \\ ∆H_f°(N_2O_{4(l)})=-20\text{ }kJ\text{/}mol \\ \\ ∆H_f°(H_2O_{(g)})=-258.8\text{ }kJ\text{/}mol \\ \\ ∆H_f°(N_{2(g)})=0\text{ }kJ\text{/}mol \\ \\ ∆H_f°(CO_{2(g)})=-393.5\text{ }kJ\text{/}mol \end{gathered}[/tex]The ∆H° for this reaction can be calculated using the formula below:
[tex]\Delta H_{rxn}\degree=ΔH_f^{\degree}(products)-ΔH_f^{\degree}(reactants)[/tex]Put the each enthalpy of formation of the reactants and the products into the formula:
[tex]\begin{gathered} \Delta H_{rxn}\degree=[12(-258.8)+9(0)+4(-393.5)]-[4(+53)+5(-20)] \\ \\ \Delta H_{rxn}\degree=[-3105.6+0-1574]-[212-100] \\ \\ \Delta H_{rxn}\degree=-4679.6-112 \\ \\ \Delta H_{rxn}\degree=-4791.6\text{ }kJ\text{/}mol \end{gathered}[/tex]Therefore, the ∆H° for this reaction is -4791.6 kJ/mol.
Calculate the number of molecules in 8.21 x 10^-2 moles in (NH4)2Cr2O7
Answer
4.94x10^22 molecules
explanation
to calculate the number of molecules in 8.21x10^-2 moles ca be determined by using Avogadros number
we know that
1 mol has 6.022x10^23 molecules
therefore,
8.21x10^-2 moles have:
(8.21x10^-2) x (6.022x10^23)
= 4.94x10^22 molecules
QUESTION 2How many moles are in 37.16 g of calcium sulfate,CaSO4
In order to find the number of moles in a given mass of any compound, we need to use the molar mass of this compound, which is the total mass present in 1 mol of the compound. The molar mass of CaSO4 is 136.14g/mol
136.14 grams = 1 mol of CaSO4
37.16 grams = x moles of CaSO4
136.14x = 37.16
x = 37.16/136.14
x = 0.27 moles of CaSO4
In 37.16 grams, we will have 0.27 moles of CaSO4
Which of the following best describes an ecosystem in the Great Lakes?
The statement " all the living organisms in an area and their physical surroundings " will describes an ecosystem in the Great Lakes.
A biological combination of cooperating organisms and surrounding physical environment can be referred to as an ecosystem.
A system made up of biotic and abiotic elements that work together as a whole is called an ecosystem. All live things are considered to be biotic components, although non-living items are considered to be abiotic components.
Therefore, "all the living organisms in an area and their physical surroundings " will define ecosystem in the Great Lakes.
The given question is incomplete. The complete question is
Which of the following best describes an ecosystem?
A. all the living organisms in an area
B. all the living organisms in an area and their physical surroundings
C. a region with a distinct climate
D. all the living organisms of the same species throughout the world
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How many grams of 12% solution can be prepared from 35 g of CaCl2
The question provides the concentration of a solution (12% CaCl2) and requests us to calculate how many grams of this solution could be prepared starting from 35g of CaCl2.
Since the concentration of solution is 12%, considering it refers to % in mass, we can write that 12g of CaCl are necessary to prepare 100 g of solution:
12 g of CaCl2 --------------- 100 g of solution
Thus, we can calculate how much solution could be prepared from 35 g of CaCl2:
12 g of CaCl2 --------------- 100 g of solution
35 g of CaCl2 -------------- x
Solving for x, we have that 291.67 g of solution could be prepared from 35g of CaCl2.
The theoretical value isa) true valueOb) experimental valueOc) observed valueO d) measured value
Answer:
[tex]A\text{ : True value}[/tex]Explanation:
Here, we want to get another name for the theoretical value
The theoretical value is simply the value that has been accepted as true
Thus, we can call the theoretical value the true value
What is the phase of water at 0.25 atm and 0°C?A. GasB. Solid and liquidC. Solid and gasD. Solid
Explanation:
We have to find the phase of water at 0.25 atm and 0°C. If we look at the phase diagram of water and throw the lines we will find that the phase of water at those conditions is solid.
Answer: d. Solid
What mass of oxygen is needed to burn 54.0 g of butane
Answer
The mass of oxygen needed to burn 54.0g of butane is 193.24 g
Explanation
Given:
Mass of butane = 54.0 g
What to find:
The mass of oxygen needed to burn 54.0g of butane.
Step-by-step solution:
Step 1: Write the balanced chemical equation for the reaction.
2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O
Step 2: Convert 54.0 g of butane to moles
Molar mass of C₄H₁₀ = 58.12 g/mol
[tex]Moles=\frac{Mass}{Molar\text{ }mass}=\frac{54.0\text{ }g}{58.12\text{ }g\text{/}mol}=0.9291\text{ }mol[/tex]Step 3: Use the mole ratio in step one and the mole of C₄H₁₀ in step 2 to calculate the mole of oxygen.
[tex]\begin{gathered} 13\text{ }mol\text{ }O_2=2\text{ }mol\text{ }C_4H_{10} \\ \\ x=0.9291\text{ }mol\text{ }C_4H_{10} \\ \\ x=\frac{0.9291\text{ }mol\text{ }C_4H_{10}}{2\text{ }mol\text{ }C_4H_{10}}\times13\text{ }mol\text{ }O_2 \\ \\ x=6.03915\text{ }mol\text{ }O_2 \end{gathered}[/tex]Step 4: Convert the moles of O₂ in step 3 to mass in grams.
Molar mass of O₂ = 31.998 g/mol
[tex]\begin{gathered} Mass=Moles\times Molar\text{ }mass \\ \\ Mass=6.03915mol\times31.998g\text{/}mol \\ \\ Mass=193.24\text{ }g\text{ }of\text{ }O_2 \end{gathered}[/tex]Hence, the mass of oxygen needed to burn 54.0g of butane is 193.24 g
The mole fraction of NaCl in anaqueous solution is 0.132. Howmany moles of water are present in1 mole of this solution?Molar MassNaCl: 58.44 g/molH2O: 18.016 g/mol
The problem is asking for how many moles of water there are in 1 mol of solution with NaCl. This is telling us that NaCl is dissolved in water.
There are 0.132 moles of NaCl and summing the moles of water, we're going to obtain 1 mol of solution. You can see it, like this:
[tex]\text{0}.132\text{ moles NaCl+X moles water = 1 mol solution.}[/tex]We just have to clear for 'X moles water', and we obtain:
[tex]X\text{ moles water = 1-0.132 = 0.868 moles water.}[/tex]The answer is that we have 0.868 moles of water in the solution.
write any three chemical properties of carbon
Answer
• Carbon has the atomic symbol C,
,• Carbon is a nonmetallic chemical element with 4 electrons in its valence shell, which allows it to form 4 bonds forming compounds like CH₄.
,• Reactivity: Carbon does not dissolve in or react with water or acids.
,• The atomic mass of carbon is 12.011 g. It contains 6 protons in its nucleus.
Balance the following half-reaction in acid (some electrons, e, will be needed to balance it):Fe²+ ——-> FeO4²-
The balanced half-reaction is Fe²⁺ + 2e⁻ --------> FeO₄²⁻
The given reaction is a redox reaction. Balancing a redox reaction is a bit different than solving a normal chemical reaction. The first step is to find the oxidation state of each element in the reactant as well as the product side. By doing so we get,
The oxidation state of Fe - +2
On the product side, we get,
The oxidation state of Fe - +6
The oxidation state of O - -2
The next step is to calculate the difference between the oxidation states.
The difference in oxidation state of Fe - +6 - (+2) = +4
The difference in oxidation state of O - 0 -2 = -2
To balance this reaction, 2 electrons should be added to the reactant side so that the oxidation states of O and Fe get balanced equally. By doing so we get,
Fe²⁺ + 2e⁻ --------> FeO₄²⁻
This is a balanced half-reaction in acid
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A balloon is filled to a volume of 1.50 L with 2.50 moles of gas at 25 °C. With pressure and temperature held constant, what will be the volume of the balloon if 0.20 moles of gas are added?
The final volume of the balloon if 0.20 moles of gas are added will be 1.62 L.
What will be the volume of the balloon given that 0.20 moles of a gas is added to it?The volume of the balloon given that 0.20 moles of a gas is added to it is determined using the ideal gas equation as follows:
P₁V = nRT
Where;
P is pressureV is volumen is the number of moles of gasR is molar gas constant = 0.082 atm.L/K.molInitial volume, V₁ = 1.50 L
Initial mole of gas, n₁ = 2.50 mol
Initial temperature, T₁= 25°C or 298 K
Initial pressure, P₁ = RT₁n₁/V₁
P₁ = 0.082 * 298 * 2.50 /1.50
P₁ = 40.7 atm
With pressure and temperature held constant:
Final temperature, T₂ is equal to T₁ = 298 K
Final pressure, P₂ is equal to P₁ = 40.7 atm
Final moles of gas, n₂ = 0.20 + 2.5
n₂ = 2.70 mol
Final volume, V₂ = RT₂n₂/P₂
V₂ = 0.082 * 298 * 2.70 /40.7
V₂ = 1.62 L
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If something is made of 2.1 g Ni and 0.58 g O, what is the empirical formula?
To know the empirical formula we will determine how many moles of each element we have. To do this, we must look up in the periodic table the atomic weight of each element.
The atomic weight of Ni = 58.6934 g/mol
O = 15.999 g/mol
Now we divide the mass of each element by its atomic weight to determine how many moles are in the sample.
[tex]\begin{gathered} \text{Mol of Ni = }\frac{\text{Mass of Ni}}{\text{Atomic weight}} \\ Mol\text{ of Ni = }\frac{\text{2.1 g}}{58.6934\text{ g/mol}}=0.036\text{ mol of Ni} \end{gathered}[/tex][tex]\begin{gathered} \text{Mol of O = }\frac{Mass\text{ of O}}{\text{Atomic weight}} \\ \text{Mol of O = }\frac{0.\text{58 g}}{15.999\text{ g/mol}}=\text{ 0.036 mol of O} \end{gathered}[/tex]In the sample, there are 0.036 moles of oxygen and 0.036 moles of Ni. The ratio is 1 to 1, so the empirical formula will be: NiO
What is the concentration if I have 450 mL of iron (II) chloride (FeCl2) solution that contains9.6 grams of iron (II) chloride solute?
0.168M
Explanations:The formula for calculating the concentration of the solution is expressed as:
[tex]concentration=\frac{mole}{volume}[/tex]Determine the moles of iron(II) chloride
[tex]\begin{gathered} mole\text{ of FeCl}_2=\frac{9.6g}{126.751g\text{/}mol} \\ mole\text{ of FeCl}_2=0.0757moles \end{gathered}[/tex]Given that volume is 0.45L, hence the concentration is expressed as:
[tex]\begin{gathered} concentration=\frac{0.0757}{0.45} \\ concentration=0.168M \end{gathered}[/tex]Hence the concentration of the solution is 0.168M
Using the ΔH -48.8 kJ/mmol, calculate the enthalpy change if you neutralized six moles of HCl with an equal number of moles NaOH to one decimal place.
-292.8J/mmol
Explanations:Given the reaction of NaCl and NaOH expressed by the chemical equation:
[tex]6HCl+6NaOH\rightarrow6NaCl+6H_2O[/tex]Amount of heat released when one mole of strong acid reacts with one mole of the strong base is -48.8 kJ/mmol.
If 6 moles of the sample acid reacts with 6 moles of NaOH, the required enthalpy cheange is expressed as:
[tex]\begin{gathered} Amount\text{ of heat released }=6\times-48.8 \\ Amount\text{ of heat released}=-292.8kJ\text{/mmol} \end{gathered}[/tex]Hence the enthalpy change if you neutralized six moles of HCl with an equal number of moles NaOH is -292.8J/mmol