The new volume will be 33.5 L.
Explanation:
The kinetic theory of gases indicates that the space occupied by gas molecules is directly proportional to their temperature while being inversely proportional to the pressure. Assuming the number of moles is n = 1, the equation for gases can be written as:
PV = nRT
In this equation, P stands for pressure, V represents volume, R is the gas constant, and T denotes temperature.
Given that P = 523 Torr, T = 7.50 °C = 7.50 + 273.15 = 280.65 K, and the gas constant R = 62.363 Torr L mol⁻¹K⁻¹.
Consequently, the new volume will be 33.5 L.
Answer:
The typical atomic weight of bromine is 79.9 amu.
Explanation:
Provided information:
Br⁷⁹ constitutes 55% of the sample
Br⁸¹ constitutes 45% of the sample
What is the average atomic weight of bromine?
Calculation formula:
Average atomic mass = [isotope mass × its proportion] + [isotope mass × its proportion] +...[ ] / 100
We can now insert the known values into the formula.
Average atomic mass = [55 × 79] + [81 × 45] / 100
Average atomic mass = 4345 + 3645 / 100
Average atomic mass = 7990 / 100
Average atomic mass = 79.9 amu
The typical atomic weight of bromine is 79.9 amu.
The amount to administer to the child is 2,469 mL.
To convert to kilograms (kg), the child's weight in pounds (lb) is multiplied by 0.45359237: m(child) = 72.6 · 0.045359237 = 32.93 kg.
To find m(Medrol), the child's mass in kilograms is multiplied by 1.5 mg/kg.
Thus, m(Medrol) = 32.93 kg · 1.5 mg/kg = 49.39 mg.
The concentration of Medrol is d(Medrol) = 20.0 mg/mL.
To find the volume of Medrol needed, use V(Medrol) = m(Medrol) ÷ d(Medrol).
So, V(Medrol) = 49.39 mg ÷ 20 mg/mL = 2,469 mL.
1 atomic mass unit (amu) represents the mass of an atom or is used to measure mass on an atomic scale. It is also referred to as a dalton, abbreviated as Da, while atomic mass unit is indicated as amu.
1 amu can be translated into grams as follows:
For conversion into grams:
Therefore, the mass of Te is 204.16 * 10^-2^4 g
Answer:
The accurate answer is 596.5 kJ.
Explanation:
The question specifies that the mass of ethanol, C2H5OH, is 20 grams.
The molar mass of ethanol is 46 g/mol.
To find the moles of ethanol, we use the formula:
n = mass / molar mass
= 20/46 = 0.435 moles
According to the question, the standard heat of combustion for ethanol is 1372 kJ/mol. Hence, one mole releases 1372 kilojoules during combustion.
The energy produced from burning 20 grams of ethanol completely is 0.435 * 1372 = 596.5 kJ.
