Answer:
177.993 MeV
Explanation:
Nuclear fission refers to a process where a nucleus is broken into smaller ones.
m(Am) = 242.0595490 u, m(Sr) = 89.9077387 u, m(La) = 148.934733 u and m(n) = 1.008665 u. To find the mass of X, we sum up the masses on both side and subtract them according to the equation given
242 + X = 90 +149 + 4
X = 243 - 242 = 1
so X is a neutron
next we calculate the Δm ( change in mass)
Δm = mass reactant - mass of product
(242.0595490 + 1.008665 ) - ( 89.9077387 + 148.934733 + 4 (1.008665))
= 243.068214 - 242.8771317 = 0.1910823 u
using the formula
E = (Δm) c² = 0.1910823 u × c² × 
× 
= 177.993 MeV
Did you perhaps mean the phase of matter?
If so, then a solution has only one phase of matter: liquid. It is always almost always liquid because solutions are made up of a solvent and a solute and a solvent is always a liquid. Though, some may come in an emulsion form, but still it can be considered as liquid
The molar mass of the gas that has a mass of 3.82 g and occupies a volume of 0.854 L is 106.66g/mol.
<h3>How to calculate molar mass?</h3>
The molar mass of a substance can be calculated by dividing the mass of the substance by its number of moles.
However, the number of moles of the gas in this question needs to be calculated first using the ideal gas law equation:
PV = nRT
Where;
- P = pressure
- V = volume
- n = number of moles
- T = temperature
- R = gas law constant
1.04 × 0.854 = n × 0.0821 × 302
0.888 = 24.79n
n = 0.888/24.79
n = 0.036mol
Molar mass of gas = 3.82g/0.036mol
Molar mass = 106.66g/mol
Therefore, the molar mass of the gas that has a mass of 3.82 g and occupies a volume of 0.854 L is 106.66g/mol.
Learn more about molar mass at: brainly.com/question/12127540
From the stoichiometry of the combustion reaction, we can see that 7.4 L of oxygen is consumed.
<h3>What is combustion?</h3>
Combustion is a reaction in which a substance is burnt in oxygen. The equation of the reaction is; C4H10O(l) + 6O2 (g) → 4CO2 (g) + 5H2O(l)
We can obtain the number of moles of CO2 from;
PV = nRT
n = 1.02 atm * 7.15 L/0.082 atm LK-1mol-1 * (125 + 273) K
n = 7.29 /32.6
n = 0.22 moles
If 6 moles of oxygen produces 4 moles of CO2
x moles of oxygen produces 0.22 moles of CO2
x = 0.33 moles
1 mole of oxygen occupies 22.4 L
0.33 moles of oxygen occupies 0.33 moles * 22.4 L/ 1 mole
= 7.4 L of oxygen
Learn more about stoichiometry: brainly.com/question/13110055
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Answer:
Explanation:
The given equation for the chemical reaction can be expressed as;
Using Hess Law to determine how much heat is produced by the decomposition of exactly 1 mole of H2O2 under standard conditions; we have the expression showing the Hess Law as follows:
At standard conditions;
the molar enthalpies of the given equation are as follows:
Replacing them into above formula; we have:
The above is the amount of heat of formation for two moles of hydrogen peroxide; thus for 1 mole hydrogen peroxide ; we have :
Hence; the heat produced after the decomposition of 1 mole of hydrogen peroxide is -54.04 kJ/mol
