Answer:
False
Explanation:
In Nuclear plants accidents such as explosions can occur which may lead to loss of life or severe injuries.
Nuclear energy production does not produce emissions but it produces radioactive waste which have to be stored adequately to prevent pollution. Since nuclear waste cannot be destroyed, measures have to be taken to adequately store the waste.
If the nuclear plant is being attacked, it can be used as a nuclear weapon to create disaster
When the amount of heat gained = the amount of heat loss
so, M*C*ΔTloses = M*C* ΔT gained
when here the water is gained heat as the Ti = 25°C and Tf= 28°C so it gains more heat.
∴( M * C * ΔT )W = (M*C*ΔT) Al
when Mw is the mass of water = 100 g
and C the specific heat capacity of water = 4.18
and ΔT the change in temperature for water= 28-25 = 3 ° C
and ΔT the change in temperature for Al = 100-28= 72°C
and M Al is the mass of Al block
C is the specific heat capacity of the block = 0.9
so by substitution:
100 g * 4.18*3 = M Al * 0.9*72
∴ the mass of Al block is = 100 g *4.18 / 0.9*72
= 19.35 g
The molar mass of the imaginary compound Z(AX₃)₂ is the sum of the molar mass of Z, A and X.
<h3>How do we calculate molar mass?</h3>
Molar mass of any compound will be calculated by adding the mass of each atoms present in that compound.
Given compound is Z(AX₃)₂, molar mass of the given compound will be calculated as:
Molar mass of Z(AX₃)₂ = Molar mass of Z + molar mass of 2(A) + molar mass of 6(X)
Hence molar mass of Z(AX₃)₂ is the sum of the masses of all atoms.
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CH3CH2OH = 46.068 (molar mass)
1.50g(1 mole / 46.0680) =
0.03256 moles
Answer:
Explanation:
As per the law of conservation of mass all the mass of carbon present in the hydrocarbon weighing 112 g is present in the 328.5 g of carbon dioxide produced when the hydrocarbon was burned in air.
<u>1) Calculate the mass of carbon in 328.5 g of carbon dioxide</u>:
- Chemical formula of carbon dioxide: CO₂
- Molar mass of CO₂: 12.011 g/mol + 2 × 15.999 g/mol = 44.009 g/mol
x / 328.5 g CO₂ = 12.011 g C / 44.009 g/mol ⇒ x = 86.65 g C
<u>2) Calculate the percent mass of carbon:</u>
- % = (mass of carbon / mass of carbon dioxide) × 100 =
= (89.65 / 112) × 100 = 80.04%
Round to three signifcant figures: 80.0%.
